The equilibrium constant, K, for the following reaction is 8.93 at 739 K. 2NH3(g) N2(g) + 3H2(g) In order to Calculate Kc at this temperature for the following reaction: 1/2N2(g) + 3/2H2(g) NH3(g) The original Kc value will need to be multiplied by 1/2. True False

At 1100 K, Kp = 0.21 for the reaction 2SO2 (g) + O2 (g) = 2SO3 (g) What is the value of K at this temperature? K =

Cl3] ² [Hz] ² [A] [AC] Consider the chemical equation and equilibrium constant for the synthesis of ammonia at 25 °C: N₂ (g) + 3 H₂ (g) = 2 NH3 (g) K = 5.6 x 105 Calculate the equilibrium constant for the following reaction at 25 °C: NH3 (g) 1/2 N₂ (g) + 3/2 H₂ (g) K' = ? Kc = [NH3 ]² [₂] [H₂]] Kc- [~₂] ¹/2 [H NH3

Consider the following equilibrium: CO(g) + 3 H2(g)⇄CH4(g) + H2O(g). If Kp = 5.25 x 10-5 at 1468.0 K, calculate Kc.

Calculate the value of K, for the equation C(s) + CO₂(g) given that at a certain temperature Kp = 2 CO(g) K₂ = ? C(s) + 2 H₂O(g) CO₂(g) + 2 H₂(g) H₂(g) + CO₂(g) = H₂O(g) + CO(g) Kpl = 3.35 Kp2 = 0.745

Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 2 NH3 (9) N₂H₁(g) + H₂ (9) Round your answer to 2 significant digits. K = 0 x10 x ⑤

For this equilibrium system, 2SO3(g) 2 25O2(g) + O2(g), Kc = 0.00407. At equilibrium, you would expect to find %3D relatively more products than reactant. relatively more reactant than products. about comparable amounts of reactant and products. no way to decide.

Do not give handwriting solution. Given the following equilibrium reaction and equilibrium constant at 300 K: 2 SO3 (g) ⇌ O2 (g) + 2 SO2 (g) Kp = 0.049 calculate the equilibrium constant (Kp) for the following reaction at the same temperature. Enter your answer with no units. 3 O2 (g) + 6 SO2 (g) ⇌ 6 SO3 (g) Kp = ?

Nitrogen dioxide decomposes according to the reaction 2 NO2 (g) ⇌ 2 NO (g) + O2 (g)  Where Kp = 4.48 x 10 ^ -13 at a certain temperature. If 0.40 atm of NO is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO (g) and O2 (g)?  P NO =   atm NO P O2 =   atm O2 Use correct significant figures.

For which of these reactions will there be no effect on the relative amounts of the substances present at equilibrium when the pressure of the system is increased at constant temperature? O 2 sO, (g) + 0,(g) = 2 SO, (g) + heat heat + CO, (g) + NO(g) =CO(g) + NO, (g) heat + 2 Cl, (g) + 2 H,O(g) = 4 HCI(g) + 0, (g) N, (g) + 3 H, (g) = 2 NH, (g) + heat