Question

H2SO4 + 8HI → H2S + 412 + 4H2O

If this reaction produces 6 moles of 12, what amount of H2SO4
was present at the beginning of the reaction?
a
b
d
1.5 moles
4 moles
2 moles
6 moles

Answer 1

The amount of H2SO4 present at the start of the reaction was calculated to be a) 1.5 moles, using the stoichiometry of the balanced chemical equation which shows a mole ratio of 1:4 between H2SO4 and I2.

Step-by-step explanation:

The balanced chemical equation given is H2SO4 + 8HI → H2S + 4I2 + 4H2O. This equation indicates that 1 mole of sulfuric acid (H2SO4) produces 4 moles of iodine (I2). If the reaction produces 6 moles of I2, we can use stoichiometry to find the amount of H2SO4 that was present at the beginning of the reaction.

Using the mole ratio from the balanced equation (1 mole H2SO4 : 4 moles I2), we can calculate the moles of H2SO4 needed to produce 6 moles of I2.

1 mole H2SO4 is to 4 moles I2 as x moles H2SO4 is to 6 moles I2:

x = × (6 moles I2) / (4 moles I2) = 1.5 moles H2SO4

Therefore, 1.5 moles of H2SO4 were present at the beginning of the reaction.