If 0.50 g of O2(g) reacts with excess H2(g), what is the volume of H2O(g) obtained from the reaction at STP?
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Answer:
The enthalpy change in the the reaction is -47.014 kJ/mol.
Explanation:
Volume of water in calorimeter = 22.0 mL
Density of water = 1.00 g/mL
Mass of the water in calorimeter = m
Mass of substance X = 2.50 g
Mass of the solution = M = 2.50 g + 22 g = 24.50 g
Heat released during the reaction be Q
Change in temperature =ΔT = 28.0°C - 14.0°C = 14.0°C
Specific heat of the solution is equal to that of water :
c = 4.18J/(g°C)
Heat released during the reaction is equal to the heat absorbed by the water or solution.
Heat released during the reaction =-1.433 kJ
Moles of substance X=
The enthalpy change, ΔH, for this reaction per mole of X: