6). Calculate the ?G°rxn for the reaction below. Note: T = 25 °C C3H8(g) + 5 O2(g) ? 3 CO2(g) + 4 H2O(l) ?G°rxn = ? CO2(g) = -394.36 kJ/mol H2O(l) = -237.1 kJ/mol CH3H8(g) = 0 kJ/mol O2 = 0 kJ/mol 298K : 3(-394.36) + 4(-237.1) - (0 + 4 * 0) ?G°rxn = -2131.48 kJ/mol 7). Question #7 is referred to the work of question #6. Is the reaction spontaneous or non-spontaneous at standard condition? a. Spontaneous b. Non-Spontaneous c. cannot make this prediction
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We are given the following information: AGf for CsHe(g) = 0 kJ/mol AGf for Oz(g) = 0 kJ/mol AGf for COz(g) = -394.36 kJ/mol AGf for HzO(l) = -237.1 kJ/mol The reaction is: CsHe(g) + 5 Oz(g) -> COz(g) + 4 HzO(l) Show more…
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Question 6 For the reaction 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) ΔH° is +25 kJ/mol and ΔS° is +253 J/K·mol. This reaction is ________. A. spontaneous only at high temperature B. nonspontaneous at all temperatures C. unable to determine without more information D. spontaneous only at low temperature E. spontaneous at all temperatures
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For a particular chemical reaction, deltaH = 4.3 kJ and deltaS = -19 J/K. Under what temperature condition is the reaction spontaneous? (Hint: Gibbs Free Energy (G) matters here. See the equation delta G = delta H - T delta S) When T < -226 K. When T < 226 K. The reaction is not spontaneous at any temperature. The reaction is spontaneous at all temperatures.
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