How much heat is produced by the complete reaction of 3.45 kg of nitromethane (C

Question

How much heat is produced by the complete reaction of 3.45 kg of nitromethane (CH_3NO_2) by the reaction: 4 CH_3NO_2(l) + 3 O_2(g) rightarrow 4 CO_2(g) + 6 H_2O(l) + 2 N_2(g) delta H_rxn = -2836 kJ 1.60 times 10^5 kJ 6.41 times 10^5 kJ 5.14 times 10^5 kJ 4.01 times l0^4 kJ 1.12 times 10^4 kJ Calculate delta H_rxn for the reaction: CH_4(g) + 4 Cl_2(g) rightarrow CCl_4(g) + 4 HCl(g) Given: C(s) + 2 H_2(g) rightarrow CH_4(g) delta H_1 = -74.6 kJ C(s) + 2 Cl_2(g) rightarrow CCl_4(g) delta H_2 = -95.7 kJ H_2(g) + Cl_2(g) rightarrow 2 HCl(g) delta H_3 = -92.3 kJ -107.3 kJ -301.4 kJ -450.6 kJ -262.6 kJ

Explanation / Answer

35)

Molar mass of CH3NO2 = 12 + 3 * 1 + 14 + 2 * 16 = 12 + 3 + 28 + 16 = 59 gm/mol

Number of moles of CH3NO2 = Mass/molar mass = 3.45 * 10^(3)/59 = 58.474 moles

Reaction uses 4 moles of CH3NO2, hence the heat produced will be

Heat Produced = 58.474/4 * Heat of Reaction

=> 14.6185 * 2836 kJ

=> 41458.066 kJ

The correct answer is Option D

36)

Given Reaction

C(s) + 2H2(g) ----- CH4(g), Delta H1 = -74.6 kJ

C(s) + 2Cl2(g) ----- CCl4(g), Delta H2 = -95.7 kJ

H2(g) + Cl2(g) ------ 2HCl(g), Delta H3 = -92.3 kJ

Desired Reaction

CH4(g) + 4Cl2(g) -----> CCl4(g) + 4HCl(g)

Multiply reaction 2 by (1) and add to 2 * Reaction 3 we get

C(s) + 4Cl2(g) + 2H2(g) ------ CCl4(g) + 4HCl(g)

Reverse the reaction 1 and add to the reaction to get the reaction

CH4(g) + 4Cl2(g) ----- CCl4(g) + 4HCl(g)

Delta H (rxn) = Delta H2 + 2 * Delta H3 - Delta H1

=> -95.7 + 2(-92.3) + 74.6

=> -205.7 kJ

Correct answer is Option E

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