At 425 ºC, Kp = 4.18 x 10 -9  for the reaction 2HBr(g) ↔ H2(g) + Br2(g) In one experiment, 0.20 atm of HBr(g), 0.010 atm H2(g) and 0.010 atm of Br2(g) are introduced into a container.  Is the reaction at equilibrium?  If not, in which direction will it proceed?

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

Some quantity of NOBr is added to an otherwise empty flask. The reaction: 2 NOBr (g) ⇄ 2 NO (g) + Br2 (g) takes place at a particular temperature for which KP  is 3.5 x 10-5. Assuming an equilibrium pressure of NOBr = 2.46atm, what is the equilibrium pressure of NO?

Consider the reaction: 2 H2S (g) ⇋ 2 H2 (g) + S2 (g) Kp = 2.4 x 10 -4 at 1073 K If the initial pressure of hydrogen sulfide is 755 torr, what will be the equilibrium partial pressure of each gas?

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.2 mol CH₄, 2.8 mol H₂S, 0.63 mol CS₂, and 0.042 mol H₂ at 93 °C. What are the values of Kc and Kp for the reaction at this temperature?   CH₄(g) + 2 H₂S(g) ⇌ CS₂(s) + 4 H₂(g)

A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(g) When she introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =

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

Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3)2 as (P NH3)2 . If either the numerator or denominator is 1, please enter 1   2 Co3O4(s)   ↔   6 CoO(s) + O2(g)

A sample of H2S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium.  What is the total pressure of all gases in the container?                             2H2S(g) ⇌ 2H2(g) + S2(g)                              Kp = 3.85 x 10-7         A sample of H2S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium.  What is the total pressure of all gases in the container?                             2H2S(g) ⇌ 2H2(g) + S2(g)                              Kp = 3.85 x 10-7         0.793 atm 0.387 atm 0.497 atm 0.215 atm 0.624 atm

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)