Consider the following equilibrium reaction: PCl5 (g) ⇌ PCl3 (s) + Cl2 (g) ΔHo = 92.5 KJ Determine the direction of the equilibrium that is favored in each of the following cases (Explain): -The temperature is raised. -Some Cl2 is added from the reaction mixture. -Some PCl3 is removed from the reaction mixture. -The pressure of the gases is decreased -A catalyst is added to the reaction mixture

The reaction is at equilibrium at some temperature, T, and the following equilibrium concentrations are measured: [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. Write the equilibrium expression for this reaction. Calculate Keq for the reaction at temperature, T.

A reaction vessel contains an equilibrium mixture of SO2, O2, and SO3. The reaction proceeds such that: 2S0, (g) +0,(g) = 2SO3 (g)

Consider the following equilibrium for which H = 180.74: N2(g) + O2(g)  2 NO(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?(a) NO(g) is added to the system.       (b) The reaction mixture is cooled.       (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e) The total pressure of the system is increased by adding a noble gas.       (f) O2(g) is removed from the system.

Heating HI(g) at 425 °C causes some of this compound to decompose, forming H2 (g) and I2 (g). Eventually, the amounts of the three species do not change further, the system has reached equilibrium. (At this point, approximately 22% of the HI has decomposed.) What is happening in this system at the molecular level? O H2(g) reacts with I2 (g) to produce HI(g) at the same rate as it decomposes. H2 (g) and I2 (g) molecules collide with HI(g) making the reaction stop. Only part of the HI(g) molecules has enough energy to decompose at this temperature. 5:55 PM FLV 2/22/2020 Type here to search hp ins prt sc delete home f12 f8 f9 f10 f5 f6 f7 14 10 num & backspace lock 23 8. 3 %24

For the following reaction, K, = 0.262 at 1000°C: C(s) + 2 H2(g) = CH4(g) At equilibrium, Pa, is 1.22 atm and 1.35 g of carbon is present. What is the equilibrium partial pressure of CH4(g)? 0.390 atm 5.68 atm 0.997 atm 0.320 atm 0.624 atm None of these

Consider the equilibrium system below. For this reaction, Kp = 205. If the equilibrium partial pressure of Cl2 is 0.050 atm and the partial pressure of NOCl is 0.095 M what is the equilibrium partial pressure of NO?   2 NO (g) + Cl2 (g) <-> 2 NOCl (g)