What is DELTAsdegree at 298 K for the following reaction? CH_4(g) + N_2(g) right

Question

What is DELTAsdegree at 298 K for the following reaction? CH_4(g) + N_2(g) rightarrow HCN(g) + NH_3(g); DELTAhdegree= 164.1 kJ; DELTAGdegree = 159.1 kJ at 298 K 2.0 J/K 550 J/K 1100 J/K 530 J/K 17 J/K for a reaction, if DELTAgdegree = 0, then which ONE of the following MUST be true? For which ONE of the following substances is the standard free energy of formation (DELTAg_fdegree) not equal to zero at 298 K? A certain reaction has negative values for both DELTAG and DELTAs. Therefore, which ONI of the statements below MUST BE correct? The reaction can be spontaneous if the temperature is low enough. The reaction cannot be spontaneous at any temperature. The reaction must be spontaneous at all temperatures. The reaction can be spontaneous if the temperature is high enough. The reaction has a positive free energy at any temperature. The standard free energy change for a chemical reaction is -6.73 kJ/mol. What is the equilibrium constant for the reaction at 25degree C? 0.0019 0.066 1.0 15 520

Explanation / Answer

7.

The equation

G = H - TS

solve for S

(G-H)/(-T) = S

S = ( H -G)/T

S = (164.1-159.1)*1000/298 = 16.77 J/K nearest is 17 J/K

NOTE Consider posting multiple questions in mutliple set of Q&A.

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.