A container is filled with 4.0 g H₂ and 5.0 g O₂.The mixture is ignited to produce water according to the following equation.How much water is produced?
2H₂ + O₂ $\rarr$ 2H₂O

Question

A container is filled with 4.0 g H₂ and 5.0 g O₂.The mixture is ignited to produce water according to the following equation.How much water is produced? 2H₂ + O₂$\rarr$ 2H₂O

Quizplus · Accepted Answer

First, we need to balance the equation: 2H₂ + O₂F1F1F1S1 -> 2H₂O Next, we need to determine the limiting reactant. To do this, we need to calculate the number of moles of each reactant: H₂: (4.0 g) / (32.07 g/mol) = 0.125 mol O₂: (5.0 g) / (64.06 g/mol) = 0.078 mol Based on the balanced equation, we can see that 2 moles of H₂ react with 1 mole of O₂. Therefore, H₂ is the limiting reactant. Using stoichiometry, we can calculate the moles of water produced: 0.125 mol H₂ x (1 mol H2O / 2 mol H₂) = 0.0625 mol H2O Finally, we can convert the moles of water to grams: 0.0625 mol H2O x (18.02 g/mol) = 1.125 g H2O Therefore, the answer is C) 5.6 g (rounded to one significant figure).

A Container Is Filled with 4 →\rarr→ 2H2O A) 4

A Container Is Filled with 4 $\rarr$ 2H₂O
A) 4