1. Warm-up: Hess’s Law and Calorimetry
Ethyne gas can undergo the following hydrogenation reaction:
C2H2(g) + 2H2(g)  C2H6(g)
a) Determine the theoretical enthalpy of hydrogenation using the equations below:
C2H2(g) + 5/2O2(g)  2CO2(g) + H2O(l) ΔH=-1300 kJ
H2(g) + ½ O2(g)  H2O(l) ΔH=-290 kJ
C2H6(g) + 7/2 O2(g)  2CO2(g) + 3H2O(l) ΔH= kJ

2. b) If g of ethyne is hydrogenated in a calorimeter with a heat capacity of 2.4 kJ/ oC that contains 20.0 kg of water, what will the change in temperature of the water and calorimeter be?