Given the following, how many grams of water could be produced in this reaction? What is the limiting reactant? If 8.7 g of water are produced, what is the percent yield?
13.74 L of hydrogen gas at 30.0 C and 801 torr and 6.53 L of oxygen gas at 25 C and 801 torr are drawn into a cylinder where the following reaction takes place:
#2H_2(g) + O_2(g) -> 2H_2O(L)#
13.74 L of hydrogen gas at 30.0 C and 801 torr and 6.53 L of oxygen gas at 25 C and 801 torr are drawn into a cylinder where the following reaction takes place:
1 Answer
WARNING! Long Answer! The theoretical yield of water is 10.1 g.
Explanation:
We have to
- use the Ideal Gas Law to calculate the moles of each gas
- identify the limiting reactant
- calculate the percent yield
- calculate the theoretical yield
Moles of
From the Ideal Gas Law,
#n = (PV)/(RT)#
∴
Moles of
∴
Identify the limiting reactant
a. Calculate the moles of
b. Calculate the moles of
The limiting reactant is
Calculate the theoretical yield of
Calculate the percentage yield