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amm1812
3 years ago
14

Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of

benzene (C6H6).
2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ
Chemistry
1 answer:
Arisa [49]3 years ago
5 0

Answer:  12033 kJ of heat produced per kg of CO_2 formed during the combustion of benzene

Explanation:

The balanced chemical equation for combustion of benzene is :

2C_6H_6(l)+15O_2(g)\rightarrow 12CO_2(g)+6H_2O(g)  \Delta H°rxn = -6278 kJ

Exothermic reactions are defined as the reactions in which energy of the product is lesser than the energy of the reactants. The total energy is released in the form of heat and \Delta H for the reaction comes out to be negative.

\text{Moles of }CO_2=\frac{\text{given mass}}{\text{Molar Mass}}=\frac{1000g}{44g/mol}=23mol      (1kg=1000g)

According to stoichiometry :

12 moles of CO_2 on combustion produce heat = 6278 kJ

Thus 23 mole of CO_2 on combustion produce heat =\frac{6278}{12}\times 23=12033kJ

Thus 12033 kJ of heat produced per kg of CO_2 formed during the combustion of benzene

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<u>Answer:</u>

<u>For Part A:</u> The partial pressure of Helium is 218 mmHg.

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To calculate the mass of helium gas, we use the equation given by ideal gas:

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P = Pressure of helium gas = 218 mmHg

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Putting values in above equation, we get:

218mmHg\times 10.2L=\frac{m}{4g/mol}\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 283K\\\\m=0.504g

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