Question

If 0.844 mol of Fe reacts with an excess of H₂O, how many moles of H₂ will be made?

A. 0.422 mol
B. 0.844 mol
C. 1.688 mol
D. 2.532 mol

If 0.99 mol of ZnCl₂ is produced, how many moles of H₂ will be produced?

A. 0.495 mol
B. 0.99 mol
C. 1.98 mol
D. 2.97 mol

How many moles of Sb4O₆ will be produced from 27.1 g of Sb and an excess of O?

A. 0.2 mol
B. 0.4 mol
C. 0.6 mol
D. 0.8 mol

117 g of HCl could make how many grams of AlCl₃?

A. 106 g
B. 117 g
C. 234 g
D. 351 g

Answer 1

The balanced equation for the reaction is Fe + 2H2O -> Fe(OH)2 + H2. Using stoichiometry, we can find that 0.844 mol of Fe will produce 1.688 mol of H2.

Step-by-step explanation:

In order to determine the moles of H₂ that will be made, we need to look at the balanced equation and use stoichiometry.
For the reaction:

Fe + 2H₂O → Fe(OH)₂ + H₂

The coefficient in front of Fe is 1, and the coefficient in front of H₂ is 2. This means that every mole of Fe will react with 2 moles of H₂O to produce 1 mole of H₂.

In the given question, 0.844 moles of Fe reacts with an excess of H₂O. Since the ratio is 1:2, we can double the number of moles of Fe to find the number of moles of H₂ that will be made.

So, 0.844 mol Fe → 0.844 x 2 = 1.688 mol H₂

Therefore, the answer is option C: 1.688 mol.