Estimate delta G degree_r times n for the following at 417 K. HCN(g) + 2 H_2(g)

Question

Estimate delta G degree_r times n for the following at 417 K. HCN(g) + 2 H_2(g) rightarrow CH_3NH_2(g) delta H degree = -158.0 kJ; delta S degree = -219.9 J/K +61.9 kJ -66.3 kJ +66.3 kJ 250 kJ +250 kJ Above what temperature does the following reaction become nonspontaneous? 2H_2S(g) + 3O_2(g) rightarrow 2 SO_2(g) + 2H_2O(g) delta H = -1036 kJ; delta S = -153.2 J/K 6.762 times 10^3 K 158.7 K 298 K This reaction is nonspontaneous at all temperatures. This reaction is spontaneous at all temperatures. Use Hess's law to calculate delta G degree r times n using the following information. ClO(g) + O_3(g) rightarrow Cl(g) + 2 O_2(g) delta G degree_r times n = ? 2 O_3(g) rightarrow 3 O_3(g) delta G degree_r times n = +489.6 kJ Cl(g) + O_3(g) rightarrow ClO(g) + O_2(g) delta G degree_r time n = -34.5 kJ -472.4 kJ 210.3 kJ +524.1 kJ +455.1 kJ +262.1 kJ The K_a of a weak acid indicator is 3.7 times 10^-7. The probable pH range of this indicator is: 6.43 to 8.43 5.

Explanation / Answer

Q11.

dG = dH - T*dS

change S from J/molK, to kJ/molK by division of 1000x

dG = (-158) - 417*(-219.9/1000)

dG = -66.30 kJ/mol

choose B

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