Which of the following is true for a particular reaction if ∆G° is -40.0 kJ/mol at 290 K and –20.0 kJ/mol at 390 K?

Calculate ΔGmix for the following mixtures at 298 K and 1.00 atm,, assuming these gases behave as ideal gases. 6.00 moles of N2,and 7.00 moles of O2 7.00 moles of CO2and 7.00 moles of N2 How do the two values compare? What does this tell us about ΔGmix?

Using the data from Appendix IIb and the data provided, compute ∆G° for the following reaction:3 CO2 (g) + Si 3 N4 (s) " 3 SiO2 (s) + 2 N2 (g) + 3 C (s, graphite)∆Gf ° (Si3 N4 (s)) = -642.6 kJ/mol.

Calculate G°, for the reaction below at 25.0 °C rxn NHẠC(s) → HCl(g) + NH3(g) given G°f [NH4CI(s)] = -202.9 kJ/mol, G°f[HCI(g)] = -95.3 kJ/mol and G°f [NH3(g)] = -16.4 kJ/mol. O +91.2 kJ O +66.7 kJ O -34.5 kJ O -133 kJ

∆G for the reaction corresponds to the difference between the top left of the curve and the bottom of the curve

A) What is the value of ∆G° for combustion of ethanol? C2H5OH(l) + 3O2(g) --> 2CO2(g) + 3H2O(l)   B) You are combusting the ethanol in an engine to do work. You need to do 450,000 J of work and the engine produces work at 23% efficiency. How many kg of ethanol do you need to combust to get the work done?

Consider 8 the following reaction: 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) ∆G° = -13.6 kJ at 25°C What is the value of ∆G at 25°C for this reaction under the following set of conditions? 25.0 atm NH3 (g) 0.500 atm CO2 (g) 1.00 M NH2CONH2 (aq) Group of answer choices -18.1 kJ 0.63 kJ -27.8 kJ 14.2 kJ -20.0 kJ

Consider the reaction: ICl(g) + Cl₂(g) → ICl₃(s). The ∆G(f)° of ICl(g) is -5.5 kJ/mol and the ∆G(f)° of ICl₃(s) is -22.59 kJ/mol What is the ∆G° of the reaction, in kJ/mol?

At 460 K, ∆G = -17.2 kJ/mol for the reaction 2 A (g) → B (g). If the partial pressures of A and B are 7.20 atm and 0.420 atm respectively, what is ∆G° for this reaction?

From the values of ΔH and ΔS predict which of the following reactions would be spontaneous at 25°C. Calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -75.8 kJ/mol,  ΔS = 126  J/K · mol