Hydrogen combines with oxygen to form water.If 1.67g of hydrogen combines with 13.33g of oxygen what mass of water will be produced?
A)1.67g
B)11.66g
C)13.33g
D)15.00g

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is:

2H2 + O2 → 2H2O

According to the equation, 2 moles of hydrogen react with 1 mole of oxygen to form 2 moles of water. The molar mass of hydrogen is 1.008 g/mol, and the molar mass of oxygen is 16.00 g/mol.

The number of moles of hydrogen in 1.67 g is:

1.67 g / 1.008 g/mol = 1.66 mol

The number of moles of oxygen in 13.33 g is:

13.33 g / 16.00 g/mol = 0.833 mol

Since oxygen is the limiting reactant, it will be completely consumed, and the amount of water formed will be determined by the amount of hydrogen available. The number of moles of water formed is:

1.66 mol H2 × (2 mol H2O / 2 mol H2) = 1.66 mol H2O

The mass of water formed is:

1.66 mol H2O × 18.02 g/mol = 29.97 g

Rounded to two significant figures, the answer is:

Answer: D (15.00 g)

Hydrogen Combines with Oxygen to Form Water