When 10.0 g of hydrogen gas reacts with 10.0 g of oxygen gas to form water, what is the theoretical yield of water?

Question

Quizplus · Accepted Answer

To determine the theoretical yield of water, we need to first balance the chemical equation for the reaction between hydrogen gas (H2) and oxygen gas (O2) to form water (H2O).

2H2 + O2 -> 2H2O

From the balanced equation, we can see that we need 2 moles of hydrogen gas to react with 1 mole of oxygen gas to form 2 moles of water.

Next, we need to convert the mass of each reactant to moles.

10.0 g of hydrogen gas = 5.0 moles of H2 
10.0 g of oxygen gas = 0.3125 moles of O2

The limiting reagent in this reaction is oxygen gas, since it is present in the smallest amount. 1 mole of O2 can produce 2 moles of H2O, so 0.3125 moles of O2 can produce:

0.3125 mol O2 x (2 mol H2O / 1 mol O2) = 0.625 mol H2O

The molar mass of water (H2O) is 18.015 g/mol, so the theoretical yield of water can be calculated as:

0.625 mol H2O x 18.015 g/mol = 11.3 g H2O

Therefore, the correct answer is C) 11.3 g.

When 100 G of Hydrogen Gas Reacts with 10