Question

How many moles of hydrogen (Upper H Subscript 2) are required to completely react with 3 moles of iron oxide (Upper F e Subscript 3 Upper O Subscript 4)?Answer options with 4 optionsA.4 molesB.6 molesC.9 molesD.12 moles

Answer 1

The balanced chemical equation for the reaction between hydrogen gas and iron oxide is:

3 Fe3O4 + 8 H2 → 9 H2O + Fe3O4

From this equation, we can see that 8 moles of hydrogen gas are required to react with 3 moles of iron oxide.

Therefore, to find how many moles of hydrogen are required to react with 3 moles of iron oxide, we can use the following proportion:

8 moles H2 / 3 moles Fe3O4 = x moles H2 / 3 moles Fe3O4

Solving for x, we get:

x = (8 moles H2 / 3 moles Fe3O4) * 3 moles Fe3O4

x = 8 moles H2

Therefore, 8 moles of hydrogen gas are required to react with 3 moles of iron oxide. The answer is not listed among the answer options provided, so there must be a mistake in the question or the answer options

Answer 2

The balanced chemical equation for the reaction of hydrogen with iron oxide is:

3H2 + Fe3O4 -> 4Fe + 4H2O

From the equation, we can see that 3 moles of hydrogen are required to react with 1 mole of iron oxide.

Therefore, to completely react with 3 moles of iron oxide, we need:

3 moles of H2 x (1 mole Fe3O4 / 3 moles H2) = 1 mole Fe3O4

Since 1 mole of Fe3O4 requires 3 moles of H2, we need:

3 moles of H2 x 1 mole Fe3O4 = 3 moles of H2

Therefore, the answer is 3 moles of hydrogen (H2).