R = 0.008314 kJ/K.mol; 1 Faraday (F) = 96, 500 C/mol e^-; 1 J = 1C times 1V. Hyd

Question

R = 0.008314 kJ/K.mol; 1 Faraday (F) = 96, 500 C/mol e^-; 1 J = 1C times 1V. Hydrazine, H_2NNH_2, is used as a rocket fuel. Use the data below to determine if hydrazine be prepared from the following reaction under standard conditions:: N_2(g) + 2 H_2(g) rightarrow H_2NNH_2(l) Calculate Delta S_total for the following reaction, then tell whether it is spontaneous under standard conditions or not. CaCO_3(s) rightarrow CaO(s) + CO_2(g) The entropy change for a certain non-spontaneous reaction at 50 degree C is 104 J/K. Is the reaction endothermic or exothermic? Explain your answer. What is the minimum value of Delta H degree (in kJ) for the reaction? Urea, NH_2CONH_2, can be prepared by the following reaction: 2 NH_3(g)+ CO_2(g) rightarrow NH_2CONH_2 (aq) Given that Delta G degree = -13.6 kJ, calculate Delta G at 25 degree C for the following set of conditions: 10 atm NH_3, 10 atm CO_2, 1.0 M NH_2CONH_2; and 0.10 atm NH_3, 0.10 atm CO_2, 1.0 M NH_2CONH_2 Would get you more product or less product for each condition?

Explanation / Answer

(1)

delta G = delta H - T delta S

delta H = products enthalpy - reactants enthalpy

= 50.63 kJ/mol

delta S = products entropy - reactants entropy

= 121.2 - ( 2 x 130.7 + 192 )

= -332.2 J/mol

delta G =  50.63 kJ/mol - (298 K x  -332.2 J/mol) == 149.62 kJ

This is positive value, so reaction is not spontaneous. This method is not used to prepare Hydrazine

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