Please show all work so that i can understand. thank you A.) Which of the follow

Question

Please show all work so that i can understand. thank you

A.) Which of the following processes have a S > 0?

B.) If G > 0, which of the following statements are true?

C.) A reaction has Hrxn=254kJ and Srxn= 201J/K.

Calculate Grxn at 41 C.

D.) Determine the equilibrium constant for the following reaction at 549 K.

CH2O(g) + 2 H2(g) CH4(g) + H2O(g) H° = -94.9 kJ; S°= -224.2 J/K

a.CH3OH(l) CH3OH(s) b.Na2CO3(s) + H2O(g) + CO2(g) 2 NaHCO3(s) c. CH4(g) + H2O(g) CO(g) + 3 H2(g) d. N2(g) + 3 H2(g) 2 NH3(g) e. All of the above processes have a S > 0.

Explanation / Answer

A )

answer : c) CH4(g) + H2O(g) CO(g) + 3 H2(g)

reason : moles of reactant = 2 , moles of products = 4 . so moles of products > moles of reactant entropy increases

B)

c) The reaction is not spontaneous.

C)

Hrxn = 254 kJ and Srxn = 201J/K.

T = 41 + 273 = 314 K

Grxn = Hrxn - T Srxn

= - 254 - 314 x 201 x 10^-3

= - 317.1 kJ

Grxn = - 317.1 kJ

D)

answer : b) 2.08 x 10^-3

Grxn = -94.9 - 549 x (-224.2 x 10^-3)

= 28.19 kJ / mol

Grxn = - R T ln Keq

28.19 = 8.314 x 10^-3 x 549 x ln Keq

Keq = 2.08 x 10^-3

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