Question

1. Calcium hydroxide, which reacts with carbon dioxide to form calcium carbonate, was used by the ancient Romans as mortar in stone structures. The reaction for this process is Ca(OH)2(s) + CO2(g) ightarrow CaCO3(s) + H2O(g) Delta H = -69.1 kJ a) What is the enthalpy change if the reaction was reversed? b) What is the enthalpy change if 3.8 mol of calcium carbonate is formed? 2. Use Hess's Law to calculate the enthalpy change for the reaction WO3 (s) + 3H2 (g) ightarrow W(s) + 3H2O(g) from the following data: 2W(s) + 3O2 (g) ightarrow 2WO3 (s) Delta H = ext{-}1685.4 kJ 2H2 (g) + O2 (g) ightarrow 2H2O(g) Delta H = -477.84 kJ

          1. Calcium hydroxide, which reacts with carbon dioxide to form calcium carbonate, was used by
the ancient Romans as mortar in stone structures. The reaction for this process is
Ca(OH)2(s) + CO2(g) 
ightarrow CaCO3(s) + H2O(g) Delta H = -69.1 kJ
a) What is the enthalpy change if the reaction was reversed?
b) What is the enthalpy change if 3.8 mol of calcium carbonate is formed?
2. Use Hess's Law to calculate the enthalpy change for the reaction
WO3 (s) + 3H2 (g) 
ightarrow W(s) + 3H2O(g)
from the following data:
2W(s) + 3O2 (g) 
ightarrow 2WO3 (s) Delta H = 	ext{-}1685.4 kJ
2H2 (g) + O2 (g) 
ightarrow 2H2O(g) Delta H = -477.84 kJ

1. Calcium hydroxide, which reacts with carbon dioxide to form calcium carbonate, was used by
the ancient Romans as mortar in stone structures. The reaction for this process is
Ca(OH)2(s) + CO2(g)
ightarrow CaCO3(s) + H2O(g) Delta H = -69.1 kJ
a) What is the enthalpy change if the reaction was reversed?
b) What is the enthalpy change if 3.8 mol of calcium carbonate is formed?
2. Use Hess's Law to calculate the enthalpy change for the reaction
WO3 (s) + 3H2 (g)
ightarrow W(s) + 3H2O(g)
from the following data:
2W(s) + 3O2 (g)
ightarrow 2WO3 (s) Delta H = ext-1685.4 kJ
2H2 (g) + O2 (g)
ightarrow 2H2O(g) Delta H = -477.84 kJ

Added by Alexa P.

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