Consider the reaction 2NH_3(g) + CO_2(g) rightarrow NH_2CONH_2(aq) + H_2O(I). Gi

Question

Consider the reaction 2NH_3(g) + CO_2(g) rightarrow NH_2CONH_2(aq) + H_2O(I). Given that delta G degree = -13.6 Kj. calculate delta G at 25 degree C for the following sets of conditions: a) 10M NH_2, 10M CO_2 1.0 M NH_2CONH_2 b) 0.10M NH_2, 0.10M CO_2, 10 M NH_2 CONH_2 State whether the following reactions are spontaneous or non-spontaneous at low, high, or all temperatures a) PCl_3(g) + Cl_2(g) rightarrow PCl_3(g) (exothermic) b) CO_2(g) + H_2(g) rightarrow CO(g) + H_2O(I) (endothermic) c) NH_3CO_2NH_2(s) rightarrow 2NH_2(g) + CO_2(g) (endothermic) Decide whether the following reactions can occur under standard conditions. Write a balanced equation for any reaction that occurs. a) oxidation of sn^2- (aq) to sn^2+ by Br_2(I) b) Reduction of Ni^2+(aq) by the oxidation of sn^2+ (aq) to sn^4+ (aq) c) Oxidation of Al(s) to Al^3+ (aq) by HCI(aq) d) Reduction of I_2(s) by the oxidation of H_2so_2Maq) to so4^2-(aq) Consider the reaction Sn^2+(aq) + 2Cl(aq) double head arrow Sn^2+(aq) + Cl_2(g) a) Calculate E^degree_cel, and the number of exchanged electrons "n". b) Calculate the equilibrium constant at 25 degree C for the reaction How many grams of chromium will be obtained when an aqueous Cr_2(so_4)_2(aq) solution is electrolyzed for 15.00 min with a constant current of2.40A? (Molar mass of Chromium 52e/mol)

Explanation / Answer

(1)

K = [NH2CONH2]/[NH3]2[CO2]

K = 1 / (10)2(10)

K = 0.001

We know that,

DeltaG = deltaG0 + RT lnK

= - 13.6 + (008314 * 298.15 * ln(0.001)

= - 30.7 kJ

(b)

K = 1 / (0.1)2(0.1)

K = 1000

DeltaG = deltaG0 + RT lnK

= - 13.6 + (008314 * 298.15 * ln(1000)

= + 3.52 kJ

(c) SInce entropy is decreased during the process,

Increase in temperature makes the reaction nonspotaneous.

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