The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K. PCl3(g) + Cl₂(g) PCI,(g) If AH for this reaction is -87.9 kJ, what is the value of Kp at 589 K?

Calculate the equilibrium constant, Kp at 640 ℃ for the reaction shown below if the standard enthalpy of reaction, ΔH°rxn = −28.0 kJ/mol at 124 ℃ and the equilibrium constant at this temperature is Kp = 30.1. CO(g) + Br2(g) ⇌ COBr2(g), ΔH = −28.0 kJ/mol R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation.

An equilibrium mixture of dinitrogen tetroxide, N2O4, and nitrogen dioxide, NO2, is 78.3% NO2 by mass at 1.00 atm pressure and 25°C. Calculate Ke at 25°C for the reaction N204 (9) = 2NO2 (g) Ke =

At -6.33 °C the concentration equilibrium constant K = 1.2 x 10 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 9.7%. • The net change in moles of gases is -2. • If the reaction is run at constant pressure, 126. kJ/mol of heat are absorbed. Using these facts, can you calculate Kat -26. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat –26. °℃ will be bigger or smaller than Kat -6.33 °C? Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No.