For each of the following balanced chemical equations, calculate how many moles of product (s) would be produced if 0.500 mole of the first reactant were to react completely.

A) CO29 (g) + 4h2 (g) = CH4 (g) + 2H2O (l)

B) BaCl2 (aq) + 2AgANO3 (aq) = 2AgCl (s) + Ba (NO3) 2 (aq)

c) C3H8 (g) + 5O2 (g) = 4H2O (l) + 3CO2 (g)

d) 3H2SO4 (aq) + 2Fe (s) = Fe2 (SO4) 3 (aq) + 3H2 (g)

A) 1.5 moles B) 1.5 moles C) 3.5 moles D) 2/3 moles

Explanation:

A) 1 mole of CO₂ gives 1 mole of CH₄ and 2 moles of H₂O, i. e, 3 moles of products. So 0.5 moles of CO₂ gives 3 x 0.5 = 1.5 moles of products.

B) 1 mole of BaCl₂ gives 2 moles of AgCl and 1 mole of Ba (NO₃) ₂, i. e, 3 moles of products. So 0.5 moles of BaCl₂ gives 3 x 0.5 = 1.5 moles of products.

C) 1 mole of C₃H₈ gives 4 moles of H₂O and 3 moles of CO₂, i. e, 7 moles of products. So 0.5 moles of C₃H₈ gives 7 x 0.5 = 3.5 moles of products.

D) 3 moles of H₂SO₄ gives 1 mole of Fe₂ (SO₄) ₃ and 3 moles of H₂, i. e, 4 moles of products. So 0.5 moles of H₂SO₄ gives 4/3 x 0.5 = 2/3 moles of products.