DHF (kJ/mol)CompoundNH:(g)CH.(g)HCN(g)H,O(g)-46.0-75.0135.1-242.06) Heat of formation values for four compounds are given in the table above.a) Calculate DHpn for the reaction 2NH;(g) + 30,(g) + 2CH,(9) → 2HCN(9) + 6H,O(g)b) Sketch an energy diagram for this change. Clearly label the reactants, products andc) As the reaction takes place, would the reaction container increase or decrease intemperature? Explain in terms of system and surroundings.d) Calculate the heat involved when 55.5 g of NH; reacts with excess oxygen andmethane.

2NH3(g) + 3O2(g)+ 2CH4(g) →2HCN(g) + 6 H2O∆H∘ = ∆Hf(products) -∆H(reactants) =(2HCN +…

Answered: DHE (kJ/mol) Compound NH (g) CH.(9)…

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DHF (kJ/mol)
Compound
NH:(g)
CH.(g)
HCN(g)
H,O(g)
-46.0
-75.0
135.1
-242.0
6) Heat of formation values for four compounds are given in the table above.
a) Calculate DHpn for the reaction 2NH;(g) + 30,(g) + 2CH,(9) → 2HCN(9) + 6H,O(g)
b) Sketch an energy diagram for this change. Clearly label the reactants, products and
c) As the reaction takes place, would the reaction container increase or decrease in
temperature? Explain in terms of system and surroundings.
d) Calculate the heat involved when 55.5 g of NH; reacts with excess oxygen and
methane.

Expert Solution

Step 1

$2 N H_{3} (g) + 3 O_{2} (g) + 2 C H_{4} (g) \to 2 H C N (g) + 6 H_{2} O ∆ H^{\circ} = ∆ H f (p r o d u c t s) - ∆ H (r e a c \tan t s) = (2 H C N + 6 H_{2} O) - (2 N H_{3} + 3 O_{2} + 2 C H_{4}) = (2 \times 135.1 + 6 \times (- 242)) - (2 \times (- 46) + 3 (0) + 2 (- 75) = - 1181.8 - (- 242) = - 939.8 K J / m o l$

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