Answer :
Final answer:
To produce 1.91 mol of water, 0.955 mol of sulfuric acid is needed, which equates to 93.65 g. The closest answer choice is 98.1 g. So , the correct option is a) 98.1 g
Explanation:
To calculate the mass of sulfuric acid (H2SO4) needed to produce 91 mol of water (H2, we can use the stoichiometry of the balanced chemical equation:
2 NaOH + H2SO4 ightarrow Na2SO4 + 2 H2O
According to the equation, 1 mol H2SO4 produces 2 mol H2 Therefore, to produce 91 mol H2O, we need half that amount in moles of H2SO4, which is 955 Using the molar mass of H2SO4 (12 g/, we can calculate the mass:
Mass H2SO4 = 955 mol imes 12 g/mol = 65 g
The closest answer choice to that is 1 g , which is likely rounded up to account for significant
