R = 0.008314 kJ/K.mol; 1 Faraday (F) = 96, 500 C/mol e^-; 1 J = 1C times 1V. Hyd
ID: 1072800 • Letter: R
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)
Hor = Hof (H2NNH2) - Hof (N2) - 2*Hof(H2)
= 50.63 - 0 - 2* 0
= 50.63 KJ/mol
= 50630 J/mol
Sor = Sof (H2NNH2) - Sof (N2) - 2*Sof(H2)
= 121.2 - 192.0 - 2* 130.7
= -332.2J/Kmol
use:
Gor = Hor - T*Sor
= 50630 - 273*(-332.2)
= 141321 J/mol
since Gor is positive, this reaction is not feasible
Answer: Cannot be prepared
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