The following sequence of reaction occurs in commercial production of aqueous nitric acid- 4NH3g-5O2g- 4NOg-6H2Ol - H-904 kJ -1 2NOg-O2g- 2NO2 g - H-112 kJ -2 3NO2g-H2Ol- 2HNO3aq-NOg - H-140 kJ -3Determine the magnitude of total heat in kJ-mole liberated at constant pressure for the production of exactly 1 mole of aqueous nitric acid by this process

4NH_3(g)+5O_2(g)→ 4NO(g)+6H_2(g) Δ H= 904 kJ ...(1) 2NO(g)+O_2(g)→ 2NO_2 (g) Δ H= 112 kJ ...(2)3NO_2(g)+H_2O(l)→ 2HNO_3(aq)+NO(g) Δ H= 140 kJ ...(3) ...

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Standard XIII

Chemistry

Heat of Reaction

The following...

Question

The following sequence of reaction occurs in commercial production of aqueous nitric acid. $4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (l) Δ H = - 904 k J . . . (1)$ $2 N O (g) + O_{2} (g) \to 2 N O_{2} (g) Δ H = - 112 k J . . . (2)$ $3 N O_{2} (g) + H_{2} O (l) \to 2 H N O_{3} (a q) + N O (g) Δ H = - 140 k J . . . (3)$
Determine the magnitude of total heat $(i n kJ/mole)$ liberated at constant pressure for the production of exactly 1 mole of aqueous nitric acid by this process

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Solution

$4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} (g) Δ H = - 904 k J . . . (1)$ $2 N O (g) + O_{2} (g) \to 2 N O_{2} (g) Δ H = - 112 k J . . . (2)$ $3 N O_{2} (g) + H_{2} O (l) \to 2 H N O_{3} (a q) + N O (g) Δ H = - 140 k J . . . (3)$
$1 mole of H N O_{3} = \frac{3}{2} moles of N O_{2} \to$
$\frac{3}{2} mole of N O \to \frac{3}{2} mole of N H_{3}$
Heat liberated to produce 1 mole of nitric acid is $\frac{3}{8} \times (Δ H_{1}) + \frac{3}{4} \times (Δ H_{2}) + \frac{1}{2} \times (Δ H_{3})$
$= (\frac{3}{2} \times \frac{1}{4}) (- 904) - (\frac{3}{2} \times \frac{1}{2}) (- 112) - (\frac{3}{2} \times \frac{1}{3}) (- 140)$
$= - 493 {kJ mol}^{- 1}$

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Similar questions

Q. The following sequence of reaction occurs in commercial production of aqueous nitric acid.

4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (l) Δ H = - 904 k J . . . (1)

2 N O (g) + O_{2} (g) \to 2 N O_{2} (g) Δ H = - 112 k J . . . (2)

3 N O_{2} (g) + H_{2} O (l) \to 2 H N O_{3} (a q) + N O (g) Δ H = - 140 k J . . . (3)

Determine the magnitude of total heat

(i n kJ/mole)

liberated at constant pressure for the production of exactly 1 mole of aqueous nitric acid by this process

If 1 mole of aqueous nitric acid is formed, calculate total heat released :

{4 N H}_{3 (g)} + {5 O}_{2 (g)} \to {4 N O}_{(g)} + {6 H}_{2} O_{g}

{2 N O}_{g} + O_{2 (g)} \to {2 N O}_{2 (g)}

{3 N O}_{2 (g)} + H_{2} O_{(g)} \to {2 H N O}_{3 (a q)} + {N O}_{(g)}

\begin{matrix} List - I & List - II (I) Dissociation of N_{2} O_{4} (g) : & (P) Increases with N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); & temperature Δ H = + 57.0 k J (II) Oxidation of N H_{3} (g) : & (Q) Decreases with 4 N H_{3} (g) + 5 O_{2} ⇌ 4 N O (g) + 6 H_{2} O (g); & pressure Δ H = - 900.0 k J (III) Oxidation of nitrogen: & (R) Increases with N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); & addition of inert Δ H = + 180.0 k J & gas at constant pressure (IV) Formation of N O_{2} (g) : & (S) Decreases with N O (g) + O_{3} (g) ⇌ N O_{2} (g) + O_{2} (g); & temperature Δ H = - 200.0 k J (T) K_{p} = K_{c} (U) K_{p} = K_{c} (R T)^{1} \end{matrix}

Which of the following options has the correct combination considering List-I and List-II?

Q. Given that:

C (s) + O_{2} (g) \to C O_{2} (g)

;

Δ H = - 394

kJ and

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

kJ and

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

;

Δ H = - 1058

kJ/mole. Using the data, the heat of formation of ethanol is:

Q. The reaction given below shows the enthalpy change for the chemical reactants between

N_{2}

O_{2}

N O

and

N O_{2}

N_{2} (g) + O_{2} (g) \to 2 N O (g) Δ H = - 110 kJ/mol

2 N O (g) + O_{2} (g) \to 2 N O_{2} (g) Δ H = - 200 kJ/mol

The correct statement among the following is/are:

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