Using the following thermochemical equation, determine the amount of heat produc

Question

Using the following thermochemical equation, determine the amount of heat produced when forming one kg of CO_2 during the combustion of benzene (C_6 H_6). 2 C_6 H_6 (i) + 15 02(g) 12 CO_2 (g) + 6 H_2 O_(g) delta H degree rxn = -6278 kJ Given the following enthalpy values for reactions at 25 degree C, what is delta H degree at 25 degree C for the following reaction: 3C_(s) + 4 H_2 (g) rightarrow C_3 H_8 (g) C(s) + O_2(g) rightarrow CO_2(g) delta H degree = -393.5 kJ C_3 H_8 (g) + 5O_2(g) rightarrow 4H_2 O(g) + 3CO_2(g) delta H degree = -2043 kJ 2H_2(g) + O_2(g) rightarrow 2H_2 O(g) delta H degree = -483.6 kJ

Explanation / Answer

q4)

the reaction is 2C6H6 + 15O2 ------> 12 CO2 + 6H2O delta H of this reaction = -6278 kJ

From this , when 12 moles of CO2 = 12 x44 g of CO2 is formed the heat produced = 6278 kJ

Thus when 0ne Kg= 1000g of CO2 is formed the heat produced = 1000x6278 /(12x44)

= 11,890kJ

Q5)

the reaction is

3C + 4H2 --------> C3H8

and the heats of combustion of C , H2 and C3H8 are given as -393.5, -241.8 and -2043 kJ respectively.

We can compute the enthalpy of reaction , when heats of combustion are given as

Heat of reaction = sum of heat of combustion of reactants - sum of heat of combustion of products

= [3(-393.5) +2(-483.6)] - (-2043)

= - 104.7 kJ

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