First, we need to calculate the enthalpy of combustion for C4H4 and C4H8 using the given enthalpies of combustion:
C4H4(g) + 5O2(g) --> 4CO2(g) + 2H2O(l)
Delta H = -2341 kJ/mol
C4H8(g) + 7O2(g) --> 4CO2(g) + 4H2O(l)
Delta H = -2766 kJ/mol
Next, we need to balance the equation for the given reaction:
C4H4(g) + 2H2(g) --> C4H8(g)
The reaction is already balanced, so we can proceed to calculate the delta H for the reaction. We can use the enthalpies of combustion for C4H4 and C4H8 to determine the delta H for the reaction:
C4H4(g) + 2H2(g) --> C4H8(g)
Delta H = (-2341 kJ/mol) + (2 * (-286 kJ/mol)) - (-2766 kJ/mol)
Delta H = -2822 kJ/mol
Therefore, the delta H for the reaction is -2822 kJ/mol.
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C4H4 (-2341 kJ/mol), C4H8 (-2766 kJ/mol) and H2 (-286 kJ/mol), calculate delta H for the reaction
C4H4(g) + 2H2(g) --> C4H8(g)
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