Question

How many grams of H2O are generated when 45.3 g O2 reacts with excess hydrogen in the stoichiometric reaction?

A) 25.5 g H2O
B) 67.8 g H2O
C) 33.9 g H2O
D) 45.3 g H2O

Answer 1

To find the mass of H2O generated when 45.3 g O2 reacts with excess hydrogen, we use the stoichiometric coefficients from the balanced equation. The answer is 50.8 g H2O.

Step-by-step explanation:

To determine how many grams of H2O are generated when 45.3 g O2 reacts with excess hydrogen in the stoichiometric reaction, we need to use the balanced equation and stoichiometry. The balanced equation is:

2H2 + O2 2H2O

From the equation, we can see that 2 moles of H2 react with 1 mole of O2 to produce 2 moles of H2O.

To find the number of moles of O2 used, we can convert the given mass of O2 to moles:

45.3 g O2 x (1 mol O2/32.0 g O2) = 1.41 mol O2

Since 1 mole of O2 reacts with 2 moles of H2O, we can calculate the number of moles of H2O produced:

1.41 mol O2 x (2 mol H2O/1mol O2) = 2.82 mol H2O

Finally, we can convert the moles of H2O to grams:

2.82 mol H2O x (18.02 g H2O/1 mol H2O) = 50.8 g H2O

Therefore, the answer is 50.8 g H2O.