When are K꜀ and Kₚ equal, and when are they not?

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Determine AG for a reaction when AG = -141.5 kJ/mol and Q = 35 at 325 K. (R = 8.314 J/mol. K)

What is AGxn (in kJ) at 1932 K for the following reaction? 2POCI3(g) → 2PC13(g) + O₂(g) POCI3(g): AH = -592.7 kJ/mol and Sº = 324.6 J/K mol) PC13(g): AH = -287.0 kJ/mol and So = 311.7 J/K mol) O₂(g): AH = ? kJ/mol and Sº = 205.0 J/K mol)

2. For the following reaction at 25°C, AG° is -118.4 kJ. At what pressure of O2 gas does AG = 0 at 25°C? 2 KCIO3 (s) + 2 KCI (s) + 3 O2 (g)

A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 129.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = -92. kJ J - 197. K AS = ? N, (g) + 3H, (g) 2NH, (3) AG = ||| kJ 2 Which is spontaneous? this reaction the reverse reaction neither

What is the increment G degree for the following reaction from the equilibrium constant at the temperature given? CaCO33(s) → CaO(s) + CO2(g)T = 900°C Kp= 1.04

Calculate ΔG for the following equation at 25.0 oC with a PH2S = 0.000100 atm, PSO2 = 0.0100 atm, PH2O = 0.0300 atm. 2H2S(g) + SO2(g) →3Srhombic(s) + 2H2O(g)   Group of answer choices -64.7 kJ/mole -50.6 kJ/mole -87.0 kJ/mole 130. kJ/mole -73.1 kJ/mole

Which pure substance under standard conditions would have the highest entropy?   O2   HCl   CH3OH   S

When 50.0 ml of 0.100 M Pb(NO3)2 solution at 20.00oC is added to 50.0 ml of 0.100 M KI solution also at 20.00oC, solid PbI2 is produced according to the equation below. The temperature of the mixture increases to 20.52oC. Calculate ΔH for the reaction below. The density of all solutions is 1.00 g/ml. The specific heat of the mixture is 4.184 J/g· oC Pb(NO3)2 (aq) + 2 KI (aq) → PbI2 (s) + 2 KNO3 (aq)