At 500 K, the reaction 2 NO(g) + Cl2(g)⇌ 2 NOCl(g) hasKp = 51. In an equilibrium mixture at 500 K, the partial pressureof NO is 0.125 atm and Cl2 is 0.165 atm. What is the partialpressure of NOCl in the equilibrium mixture? (a) 0.13 atm(b) 0.36 atm (c) 1.0 atm (d) 5.1 x 10-5 atm (e) 0.125 atm

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures cording to the reaction: PCIs(g) PC13(g) + Cl2(g) At 350°C, 0.675 M PCI s is added to a flask. If Ke=2.50, what are the equilibrium concentrations of each gas?

Consider the equilibrium between SO₂Cl₂, SO₂ and Cl₂. SO₂Cl₂(g) SO₂(g) + Cl₂(g) K 0.193 at 390 K The reaction is allowed to reach equilibrium in a 5.80-L flask. At equilibrium, [SO₂Cl₂] = 0.290 M, [SO₂] = 0.237 M and [Cl₂] = 0.237 M. (a) The equilibrium mixture is transferred to a 11.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 11.6-L flask. [SO₂Cl₂] = [SO₂] [Cl₂] = M

R Manipulating Equilibrium Constant Expressions equilibrium constant for the following reaction is 63.3 at 378 °C. K 63.3 at 378 °C H₂(g) + 12(g) = 2 HI(g) culate the equilibrium constant for the following reactions at 378 °C. a) 2 HI(g) = H₂(g) + I2(g) K = (b) HI(g) 1/2 H₂(g) + 1/2 I2(g) Show Approach Show Tutor Steps Submit Submit Answer Try Another Version K = [References] 4 item attempts remaining Previous Next

The overall reaction for photosynthesis can be represented by the following equation:       Heat + 6 CO2(g) + 6 H2O (l) ⇌C6H12O6(s) + 6 O2(g) (a)How will the following changes cause the reaction to shift: right, left, no change? (b)Increase the concentration of O2 (c)Add C6H12O6

The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + 02 (g) 2 NO (g) K, = 0.0290 at 2400°C If the initial partíal pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). 0.112 atm (A) (B) 0.0290 atm (C) 0.688 atm (D) 0.0563 atm (E) 0.0611 atm

Assume that the change in pressure of H2S is small enough to be neglected in the following problem. (a) Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition of H2S with an initial pressure of 0.824 atm. 2H2S(g)⇌2H2(g)+S2(g)KP=2.2×10−62H2S(g)⇌2H2(g)+S2(g)KP=2.2×10−6 (b) Confirm that the change is small enough to be neglected.

3. For the following reaction at equilibrium, 2BrNO(g) → 2NO(g) + Br2(g), what will happen if the volume of the container is decreased? (a) The reaction remains unchanged (b) The reaction will shift to the left (c) The reaction will shift to the right

At 400°C the reaction BaO2(s) + 4 HCI(g) 2 BaCl,(s) + 2 H,O(g) + Cl2(g) has an equilibrium constant equal to K1. How is K¡ related to the equilibrium constant K, of the reaction 2 Cl2(g) + 4 H,O(g) + 2 BaCl2(s) 2 8 HCl(g) + 2 BaO2(s) at 400°C?

Water gas is a 1:1 mixture of carbon monoxide and hydrogen gas and is called water gas because it is formed from steam and hot carbon in the following reaction: H2 O(g) + C(s) ⇌ H2(g) + CO(g). Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and hydrogen at high temperature and pressure in the presence of a suitable catalyst.(a) Write the expression for the equilibrium constant (Kc) for the reversible reaction2H2(g) + CO(g) ⇌ CH3 OH(g)                                ΔH = −90.2 kJ(b) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more H2 is added?(c) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CO is removed?(d) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CH3OH is added?(e) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if the temperature of the system is increased?(f) What will happen to the concentrations of H2, CO,…