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

Question

Using the following thermochemical equation, determine the amount of heat produced when 1.00 x 10^3 g of CO2 formed during the combustion of benzene(C6H6). 2 C6H6(l) + 15 O2(g) —> 12 CO2(g) + 6 H2O(g) delta H rxn =-6278. Explain your thought process. Using the following thermochemical equation, determine the amount of heat produced when 1.00 x 10^3 g of CO2 formed during the combustion of benzene(C6H6). 2 C6H6(l) + 15 O2(g) —> 12 CO2(g) + 6 H2O(g) delta H rxn =-6278. Explain your thought process. 2 C6H6(l) + 15 O2(g) —> 12 CO2(g) + 6 H2O(g) delta H rxn =-6278. Explain your thought process.

Explanation / Answer

Molar mass of CO2 = 1*MM(C) + 2*MM(O)

= 1*12.01 + 2*16.0

= 44.01 g/mol

mass of CO2 = 1000 g

we have below equation to be used:

number of mol of CO2,

n = mass of CO2/molar mass of CO2

=(1000.0 g)/(44.01 g/mol)

= 22.72 mol

from reaction,

when 12 mol of CO2 reacts, heat produced = 6278 KJ

So,

for 22.72 mol, heat produced = 6278*22.72/12 = 1.19*10^4 KJ

Answer: 1.19*10^4 KJ

Feel free to comment below if you have any doubts or if this answer do not work

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