Stoichiometry - AP Chemistry
Card 0 of 725
When the equation for the reaction shown below is balanced with the lowest whole-number coefficients, what is the sum of the coefficients of the reactants?
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When the equation for the reaction shown below is balanced with the lowest whole-number coefficients, what is the sum of the coefficients of the reactants?
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The coefficients of the equation, when balanced, should be 2, 13, 10, and 8. This problem wants to know the sum of the reactants, so only the coefficients on the left side of the reactants should be added. The sum of 2 and 13 is 15, so 15 is the correct answer.
The coefficients of the equation, when balanced, should be 2, 13, 10, and 8. This problem wants to know the sum of the reactants, so only the coefficients on the left side of the reactants should be added. The sum of 2 and 13 is 15, so 15 is the correct answer.
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Suppose that 8 grams of of hydrogen gas and 16 grams of oxygen gas are ignited. What is the theoretical yield, in grams, of water? Assume hydrogen has an atomic mass of 1 and oxygen has an atomic mass of 16.
Suppose that 8 grams of of hydrogen gas and 16 grams of oxygen gas are ignited. What is the theoretical yield, in grams, of water? Assume hydrogen has an atomic mass of 1 and oxygen has an atomic mass of 16.
First, convert from grams to moles using the molar masses of the compounds. There are 4 mol of hydrogen gas and 0.5 mol of oxygen gas. Oxygen gas is clearly the limiting reagent (since there is more than twice as much hydrogen gas as oxygen gas), which means that the theoretical yield of water is
Water contains two hydrogen atoms and an oxygen atom, so it has a molar mass of
Hence, 1 mol of water would have a mass of 18 g.
First, convert from grams to moles using the molar masses of the compounds. There are 4 mol of hydrogen gas and 0.5 mol of oxygen gas. Oxygen gas is clearly the limiting reagent (since there is more than twice as much hydrogen gas as oxygen gas), which means that the theoretical yield of water is
Water contains two hydrogen atoms and an oxygen atom, so it has a molar mass of
Hence, 1 mol of water would have a mass of 18 g.
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What is the mass percent of chromium in 
?
Use the values in the following table for the atomic masses of the elements shown.
What is the mass percent of chromium in 
Use the values in the following table for the atomic masses of the elements shown.
In order to find the mass percent of a certain atom in a particular molecule, you must know the mass the atom contributes to the molecule and the total mass of the molecule. In this case we calculate the mass percent using the equation
Calculating the mass of 
in the molecule is done by multiplying the atomic mass of a 
atom by the number of atoms of that element present in the molecule. There are six 
atoms in the presented molecule. We can tell this because 
has a subscript of 2 and is contained in a set of parentheses that has a subscript of 3. This tells us that there are three sets of two 
atoms in each of the molecules. The atomic mass of a 
atom is given as 52.00 amu, so we can multiply:
Now we need to calculate the total atomic mass of the molecule. We can do this by identifying the atomic mass of each element in the molecule, multiplying it by the number of that type of atom in the molecule, and summing the results together.
We then plug in the values into equation to find the mass percent.
In order to find the mass percent of a certain atom in a particular molecule, you must know the mass the atom contributes to the molecule and the total mass of the molecule. In this case we calculate the mass percent using the equation
Calculating the mass of 
Now we need to calculate the total atomic mass of the molecule. We can do this by identifying the atomic mass of each element in the molecule, multiplying it by the number of that type of atom in the molecule, and summing the results together.
We then plug in the values into equation to find the mass percent.
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Octane, 
, is an important of component of gasoline, which can be burned as fuel in cars. The following is an unbalanced equation for the combustion of octane.
If 114 g of octane are burned in the complete combustion reaction shown below, how many grams of water will be produced?
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Octane,
If 114 g of octane are burned in the complete combustion reaction shown below, how many grams of water will be produced?
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First, the equation should be balanced. This can be done with the coefficients 2, 25, 16, and 18.
Next, calculating the molar mass of octane shows that it has a molar mass of 114 g/mol. This means that 1 mole of octane is used in the reaction, and 9 times as many moles of water should be produced, meaning one of the products will be 9 mol of water. Water has a molar mass of 18 g/mol, so the total mass of water produced is 
.
First, the equation should be balanced. This can be done with the coefficients 2, 25, 16, and 18.
Next, calculating the molar mass of octane shows that it has a molar mass of 114 g/mol. This means that 1 mole of octane is used in the reaction, and 9 times as many moles of water should be produced, meaning one of the products will be 9 mol of water. Water has a molar mass of 18 g/mol, so the total mass of water produced is
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Suppose that 4 moles of 
undergoes complete decomposition. At STP, how many liters of 
would be produced as product? (At STP, one mole of a gas takes up 22.4 L of space.)
Suppose that 4 moles of
Start by creating a skeleton equation for the decomposition reaction:
This can be balanced to give:
This means that 4 mol of reactant would produce 6 mol of oxygen gas. The question states that at STP, one mole of a gas takes up 22.4 L of space, so it is easy to find that 6 moles of oxygen gas would occupy a volume of 134.4 L:
Start by creating a skeleton equation for the decomposition reaction:
This can be balanced to give:
This means that 4 mol of reactant would produce 6 mol of oxygen gas. The question states that at STP, one mole of a gas takes up 22.4 L of space, so it is easy to find that 6 moles of oxygen gas would occupy a volume of 134.4 L:
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What determines the amount of product formed in an irreversible reaction?
What determines the amount of product formed in an irreversible reaction?
In irreversible reactions, the reaction proceeds in one direction only and these reactions usually go to completion. Since the forward reaction is the only one that occurs, the amount of product formed is only based on the reactants present, namely, the amount of limiting reactant.
In irreversible reactions, the reaction proceeds in one direction only and these reactions usually go to completion. Since the forward reaction is the only one that occurs, the amount of product formed is only based on the reactants present, namely, the amount of limiting reactant.
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Balance the following equation:
FeCl3 + NOH5 → Fe(OH)3 + NH4Cl
Balance the following equation:
FeCl3 + NOH5 → Fe(OH)3 + NH4Cl
The first thing to do is to balance the Cl (3 on the left; one on the right) ← add 3 for NH4Cl
Now, there are 3 N on the right and only one on the left; add a 3 to the NOH5
Check to see that the Fe, H, and O balance, which they do
The first thing to do is to balance the Cl (3 on the left; one on the right) ← add 3 for NH4Cl
Now, there are 3 N on the right and only one on the left; add a 3 to the NOH5
Check to see that the Fe, H, and O balance, which they do
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Balance the following equation:
NaOH + H2SO4 → H2O + Na2SO4
Balance the following equation:
NaOH + H2SO4 → H2O + Na2SO4
Balancing equations:
there is 1 NaOH and 1 H2SO4 in the reactants; and 1 H2O and 1 Na2SO4 in the products
steps:
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balance the Na first; get 2 NaOH
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balance H next; get 1 H2SO4, 2 H2O
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check to make sure that O and S balance
Balancing equations:
there is 1 NaOH and 1 H2SO4 in the reactants; and 1 H2O and 1 Na2SO4 in the products
steps:
-
balance the Na first; get 2 NaOH
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balance H next; get 1 H2SO4, 2 H2O
-
check to make sure that O and S balance
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_Fe2O3 + _HCl ⇌ _FeCl3 + _H2O
The Following question will be based on the unbalanced reaction above
For the reaction above to be balanced what coefficient should be in front of the compound HCl?
_Fe2O3 + _HCl ⇌ _FeCl3 + _H2O
The Following question will be based on the unbalanced reaction above
For the reaction above to be balanced what coefficient should be in front of the compound HCl?
Balancing reactions is best acheived by using a stepwise approach. It is useful to work through each atom making sure it is present in a balanced fashion on both sides of the equation. Starting with Fe, Fe2O3 is the only molecule with Fe present on the left side of the equation and FeCl3 is the only molecule with Fe present on the right side of the equation. Thus the molar ratio of Fe2O3 to FeCl3 must be 1:2. Moving on to O, the O on the left side of the equation exists as Fe2O3 and H2O on the right. The molar ratio of Fe2O3 to H2O is therefore 1:3. Cl exists in HCl on the left and FeCl3 on the right. Thus the molar ratio of HCl to FeCl3 must be 3:1. To ensure that these molar ratios are maintaned the balanced formula is then determined to be Fe2O3 + 6HCl -> 2FeCl3 + 3H2O
Balancing reactions is best acheived by using a stepwise approach. It is useful to work through each atom making sure it is present in a balanced fashion on both sides of the equation. Starting with Fe, Fe2O3 is the only molecule with Fe present on the left side of the equation and FeCl3 is the only molecule with Fe present on the right side of the equation. Thus the molar ratio of Fe2O3 to FeCl3 must be 1:2. Moving on to O, the O on the left side of the equation exists as Fe2O3 and H2O on the right. The molar ratio of Fe2O3 to H2O is therefore 1:3. Cl exists in HCl on the left and FeCl3 on the right. Thus the molar ratio of HCl to FeCl3 must be 3:1. To ensure that these molar ratios are maintaned the balanced formula is then determined to be Fe2O3 + 6HCl -> 2FeCl3 + 3H2O
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After the following reaction is balanced, how many moles of H2O can 4 moles of C2H6 produce?
__C2H6(s) +
O2(g) →
H2O(l) +
CO2(g)
After the following reaction is balanced, how many moles of H2O can 4 moles of C2H6 produce?
__C2H6(s) + O2(g) → H2O(l) + CO2(g)
The reaction balances out to 2C2H6(s) + 7O2(g) → 6H2O(l) + 4CO2(g). For every 2 moles of C2H6 you can produce 6 moles of H2O. Giving you a total production of 12 moles when you have 4 moles of C2H6.
The reaction balances out to 2C2H6(s) + 7O2(g) → 6H2O(l) + 4CO2(g). For every 2 moles of C2H6 you can produce 6 moles of H2O. Giving you a total production of 12 moles when you have 4 moles of C2H6.
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Consider the following unbalanced equation for the combustion of propane, 
:
If you were to combust one mole of propane, how many moles of water would you produce?
Consider the following unbalanced equation for the combustion of propane,
If you were to combust one mole of propane, how many moles of water would you produce?
Begin by balancing the equation. There are many ways to do this, but one method that is particularly useful is to assume that you have 1 mole of your hydrocarbon (propane), and balance the equation from there. It may be necessary to manipulate an equation further if you end up with fractions, but all you will need to do is multiply by an integer if that is the case.
First, we will balance the carbons. There are three carbons in propane, so we will make sure there are three carbons on the right side of the arrow as well:
This is not complete. We will next balance the hydrogens. There are eight hydrogens on the left side of the equation, so:
The last step is to balance the oxygens on the left and right side of the equation
Our equation is balanced and all coefficients are integers. If we begin with one mole of propane, we will produce four moles of water.
Begin by balancing the equation. There are many ways to do this, but one method that is particularly useful is to assume that you have 1 mole of your hydrocarbon (propane), and balance the equation from there. It may be necessary to manipulate an equation further if you end up with fractions, but all you will need to do is multiply by an integer if that is the case.
First, we will balance the carbons. There are three carbons in propane, so we will make sure there are three carbons on the right side of the arrow as well:
This is not complete. We will next balance the hydrogens. There are eight hydrogens on the left side of the equation, so:
The last step is to balance the oxygens on the left and right side of the equation
Our equation is balanced and all coefficients are integers. If we begin with one mole of propane, we will produce four moles of water.
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Consider the following unbalanced equation:
How many grams of solid iron are needed to make 36.0g of 
? Assume that chlorine is in excess.
Consider the following unbalanced equation:
How many grams of solid iron are needed to make 36.0g of
First, we will balance the equation:
Since chlorine is in excess, we know that the limiting reagent is iron.
First, we will balance the equation:
Since chlorine is in excess, we know that the limiting reagent is iron.
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Consider the following reaction:
When the equation is balanced, what will be the coefficient in front of HCl?
Consider the following reaction:
When the equation is balanced, what will be the coefficient in front of HCl?
When balancing equations, the goal is to make sure that the same atoms, in both type and amount, are on both the reactant and product side of the equation. A helpful approach is to write down the number of atoms already on both sides of the unbalanced equation. This way, you can predict which compounds need to be increased on which side in order to balance the equation. It also helps to balance oxygen and hydrogen last in the equation.
In this reaction, we can balance as follows.
Reactants: 1K, 1Mn, 1Cl, 4O, 1H
Products: 1K, 1Mn, 5Cl, 1O, 2H
So, we will need to increase H2O and HCl. The final balanced equation is written below.
When balancing equations, the goal is to make sure that the same atoms, in both type and amount, are on both the reactant and product side of the equation. A helpful approach is to write down the number of atoms already on both sides of the unbalanced equation. This way, you can predict which compounds need to be increased on which side in order to balance the equation. It also helps to balance oxygen and hydrogen last in the equation.
In this reaction, we can balance as follows.
Reactants: 1K, 1Mn, 1Cl, 4O, 1H
Products: 1K, 1Mn, 5Cl, 1O, 2H
So, we will need to increase H2O and HCl. The final balanced equation is written below.
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Balance the following chemical equation.
Balance the following chemical equation.
To balance an equation, we need to make sure there is the same amount of elements to the left of the arrow as there is to the right. We also need all the charges to balance out. We notice right away that there are three chlorine atoms on the left, but only one on the right.
(1Na, 1O, 1H, 1Fe, 3Cl : 1Na, 3O, 3H, 1Fe, 1Cl)
We can solve this by multiplying NaCl by three.
(1Na, 1O, 1H, 1Fe, 3Cl : 3Na, 3O, 3H, 1Fe, 3Cl)
This causes us to have an imbalance of sodium, which we can correct by manipulating NaOH.
(3Na, 3O, 3H, 1Fe, 3Cl : 3Na, 3O, 3H, 1Fe, 1Cl)
This is the final balanced equation. Note that it is usually easiest to manipulate oxygen and hydrogen last, since they are often involved in multiple molecules.
To balance an equation, we need to make sure there is the same amount of elements to the left of the arrow as there is to the right. We also need all the charges to balance out. We notice right away that there are three chlorine atoms on the left, but only one on the right.
We can solve this by multiplying NaCl by three.
This causes us to have an imbalance of sodium, which we can correct by manipulating NaOH.
This is the final balanced equation. Note that it is usually easiest to manipulate oxygen and hydrogen last, since they are often involved in multiple molecules.
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Calcium hydroxide is treated with hydrochloric acid to produce water and calcium chloride. Write a balanced chemical reaction that describes this process.
Calcium hydroxide is treated with hydrochloric acid to produce water and calcium chloride. Write a balanced chemical reaction that describes this process.
Calcium is in the second group of the periodic table, and is therefore going to have a 
oxidation number. Hydroxide ions have a 
charge. Calcium hydroxide will have the formula 
.
Chloride ions have a 
charge and hydrogen ions have a 
charge. The formula for hydrochloric acid is 
.
On the products side, water has the formula 
and calcium chloride has the formula 
.
Now that we know all of the formulas, we can write our reaction:
In order to balance the chloride atoms, we need to add coefficients.
Calcium is in the second group of the periodic table, and is therefore going to have a
Chloride ions have a
On the products side, water has the formula
Now that we know all of the formulas, we can write our reaction:
In order to balance the chloride atoms, we need to add coefficients.
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In the balanced version of the preceding equation, what is the coefficient of nitrogen dioxide?
In the balanced version of the preceding equation, what is the coefficient of nitrogen dioxide?
In the balanced version of the equation:
Nitrogen dioxide's coefficient is 6 in order to balance the 6 moles of nitrogen provided by the 6 moles of nitric acid on the equation's left side.
In the balanced version of the equation:
Nitrogen dioxide's coefficient is 6 in order to balance the 6 moles of nitrogen provided by the 6 moles of nitric acid on the equation's left side.
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Transesterification is an industrially important process for the production of biodiesel fuel (that most diesel engines can run cleanly on) and glycerin from triglycerides (usually people use vegetable oil as their feedstock).
One easy to do and high yielding method involves the reaction of ethanol or methanol with sodium hydroxide to produce the super bases sodium ethoxide or sodium methoxide respectively. The super base is then used in the transesterification reaction with triglycerides to produce glycerin and ethyl or methyl esters (biodiesel). The products can easily be separated by differences in density. Note: For this reaction to occur the reactants must be free of water as when water is present saponification occurs (how soap is made) which will compete with the transesterification reaction. Note: just because the reaction described above is easy doesn't mean that it is anywhere near safe; please do thoroughly research any reaction you plan to undertake and take all possible safety precautions. That being said, this process is becoming much more popular lately and with the recent focus on alternative energy may well soon account for a decent portion of fuel production.
Catalyst formation equation:
Unbalanced transesterification equation:
Balance the following transesterification reaction assuming that all R-groups are identical:
Transesterification is an industrially important process for the production of biodiesel fuel (that most diesel engines can run cleanly on) and glycerin from triglycerides (usually people use vegetable oil as their feedstock).
One easy to do and high yielding method involves the reaction of ethanol or methanol with sodium hydroxide to produce the super bases sodium ethoxide or sodium methoxide respectively. The super base is then used in the transesterification reaction with triglycerides to produce glycerin and ethyl or methyl esters (biodiesel). The products can easily be separated by differences in density. Note: For this reaction to occur the reactants must be free of water as when water is present saponification occurs (how soap is made) which will compete with the transesterification reaction. Note: just because the reaction described above is easy doesn't mean that it is anywhere near safe; please do thoroughly research any reaction you plan to undertake and take all possible safety precautions. That being said, this process is becoming much more popular lately and with the recent focus on alternative energy may well soon account for a decent portion of fuel production.
Catalyst formation equation:
Unbalanced transesterification equation:
Balance the following transesterification reaction assuming that all R-groups are identical:
The steps for balancing equations are as follows and should be done in order:
1.) Check for diatomic molecules: In this case there are none so move on to step 2
2.) Balance the metals (hydrogen is not considered a metal in this application): We have no metals in our equation, so move on to step 3 (the sodium is part of the catalyst so we don't consider it part of the balancing).
3.) Balance the nonmetals (not including oxygen). If you notice the left hand side of the equation has 3R groups and the right hand side only has one R-group. To fix this we can put a coefficient of 3 in front of 
on the right hand side giving us the following:
On the left hand side of the equation we have 7 carbon atoms but on the right hand side we have 9 carbon atoms. This can be rectified by putting a coefficient of 3 in front of 
on the left hand side of the equation giving us the following:
Now all the nonmetals (excluding oxygen) have been balanced and we can move on to step 4
4.) Balance oxygen. There are 9 oxygen atoms on both sides of the equation. Move on to step 5
5.) Balance Hydrogen. There are 17 hydrogens on both sides of the equation.
6.) Recount all atoms to make sure you have balanced correctly. 9 carbons on both sides, 3 R-groups on both sides, 9 oxygen on both sides, and 17 hydrogens on both sides.
If this problem had involved ionic species you would also want to make certain that the charges are balanced on both sides of the equation.
The charges on both sides add up to zero so your equation is balanced:
The steps for balancing equations are as follows and should be done in order:
1.) Check for diatomic molecules: In this case there are none so move on to step 2
2.) Balance the metals (hydrogen is not considered a metal in this application): We have no metals in our equation, so move on to step 3 (the sodium is part of the catalyst so we don't consider it part of the balancing).
3.) Balance the nonmetals (not including oxygen). If you notice the left hand side of the equation has 3R groups and the right hand side only has one R-group. To fix this we can put a coefficient of 3 in front of
On the left hand side of the equation we have 7 carbon atoms but on the right hand side we have 9 carbon atoms. This can be rectified by putting a coefficient of 3 in front of
Now all the nonmetals (excluding oxygen) have been balanced and we can move on to step 4
4.) Balance oxygen. There are 9 oxygen atoms on both sides of the equation. Move on to step 5
5.) Balance Hydrogen. There are 17 hydrogens on both sides of the equation.
6.) Recount all atoms to make sure you have balanced correctly. 9 carbons on both sides, 3 R-groups on both sides, 9 oxygen on both sides, and 17 hydrogens on both sides.
If this problem had involved ionic species you would also want to make certain that the charges are balanced on both sides of the equation.
The charges on both sides add up to zero so your equation is balanced:
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Consider the following unbalanced reaction:
Once this equation has been balanced, what are the the respective stoichiometric coefficients (listed in the order in which the above compounds appear in the reaction)?
Consider the following unbalanced reaction:
Once this equation has been balanced, what are the the respective stoichiometric coefficients (listed in the order in which the above compounds appear in the reaction)?
To balance chemical reactions, it's usually more effective to save the more common elements, such as oxygen, for last. For this reaction, let's go ahead and start by balancing the element 
on both sides.
Because there are 
moles of 
on the right side, we'll need to have 
moles of 
. Next, let's go ahead and balance nitrogen on both sides.
Since we added a coefficient of 
to the 
in the first step, there are now 
moles of 
on the left. Thus, we'll need to add a coefficient of 
to the 
. Next, if we check the amount of 
, 
, and 
on both sides, we see that they are equal. Thus, we can recognize that 
and 
have coefficients of 
, and do not need to be altered.
Our final balanced equation looks like this.
To balance chemical reactions, it's usually more effective to save the more common elements, such as oxygen, for last. For this reaction, let's go ahead and start by balancing the element
Because there are
Since we added a coefficient of
Our final balanced equation looks like this.
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Consider the following balanced reaction:
2Ca(s) + O2(g) → 2CaO
Consider the reaction above. If 60g of Ca is placed in a reaction chamber with 32g of O2 which will be the limiting reactant?
Consider the following balanced reaction:
2Ca(s) + O2(g) → 2CaO
Consider the reaction above. If 60g of Ca is placed in a reaction chamber with 32g of O2 which will be the limiting reactant?
When considering Limiting Reactant problems the most important aspect to consider is the molar ratio of the reactants. Here the balanced formula tells us that for every 2 moles of Ca there must be 1 mole of O2 to create the product. The amounts given by the problem are the actual amounts we are given and can be compared to the molar ratio to determine the limiting reactant. Since there is 1 mole of O2, in any situation in which there are less than 2 moles of Ca, Ca is the limting reactant. Conversely if there were 2 moles of Ca, any situation in which there less than 1 mole of O2 would be a situation in which O2 is the limiting reactant.
When considering Limiting Reactant problems the most important aspect to consider is the molar ratio of the reactants. Here the balanced formula tells us that for every 2 moles of Ca there must be 1 mole of O2 to create the product. The amounts given by the problem are the actual amounts we are given and can be compared to the molar ratio to determine the limiting reactant. Since there is 1 mole of O2, in any situation in which there are less than 2 moles of Ca, Ca is the limting reactant. Conversely if there were 2 moles of Ca, any situation in which there less than 1 mole of O2 would be a situation in which O2 is the limiting reactant.
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Given the reaction
H2SO4 (aq) + 2 LiOH (aq) → Li2SO4 (aq) + 2 H2O (l)
If you have 100g of H2SO4 and 65g of LiOH. What is your limiting reactant?
Given the reaction
H2SO4 (aq) + 2 LiOH (aq) → Li2SO4 (aq) + 2 H2O (l)
If you have 100g of H2SO4 and 65g of LiOH. What is your limiting reactant?
H2SO4 molecular weight is 98. This gives 1.02moles. Since only 1 mole is needed per reaction it allows the reaction to go through 1.02 times.
LiOH molecular weight is 24. This gives 2.71 moles. Every reaction requires 2 moles so the reaction can go through 1.35 times.
Based on this, H2SO4 is the limiting reactant.
H2SO4 molecular weight is 98. This gives 1.02moles. Since only 1 mole is needed per reaction it allows the reaction to go through 1.02 times.
LiOH molecular weight is 24. This gives 2.71 moles. Every reaction requires 2 moles so the reaction can go through 1.35 times.
Based on this, H2SO4 is the limiting reactant.
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