Calculate a value for the equilibrium constant for the reaction O2(g) + O(g) 03 (9) given hv NO(g) + O(g) K = 8.2 × 10-4⁹ NO₂(g) + O2(g) K = 7.5 × 10-34 NO₂ (g) 03 (9) + NO(g) (Hint: When reactions are added together, the equilibrium expressions are multiplied.) K=

Given the folowing equilibria: cog) + 2 H2(g) = CH;OH(g) H20(g) + C(s) = H2(g) + Co(g) K= 10. x 10-5 K= 6.0 x 10-5 What is the equilibrium constant for the following reaction? C(s) + H2(g) + H,0(g) = CH;OH(g) K = ? A. 1.6 x 104 В. 6.0 x 10-5 C. 1.6 x 10-9 D. 6.0 x 10-10 Е. 6.0 x 10-9

Write the equilibrium constant expression, K, for the following reaction: (If either the numerator or denominator is blank, please enter 1.) COC12 (g) CO(g) + Cl₂ (g) K =

3. If the equilibrium constant K, for the reaction 2 NO (g) + O2(g) = 2 NO2 (g) is 5.0 x 1012 at a given temperature, what is the value of the equilibrium constant K, for each of the following reactions at the same temperature? a) NO (g) + ½ O2 (g) → NO2 (g) b) 2 NO2 (g) = 2 NO (g) + 02 (g) c) NO2(g) = NO (g) + ½ 02 (g)

At a particular temperature, K = 1.00 x 10² for the reaction H₂(g) +1₂(g) → 2HI(g) In an experiment, 1.00 mol H₂, 1.00 mol 12, and 1.00 mol HI are introduced into a 1.00 L container. Calculate the equilibrium concentrations of all reactants and products.

The equilibrium constant, Kc, is given for one of the reactions below. What is the value of the missing equilibrium constant, Kc? Cl₂(g) + H₂O(g) = 2 HCl(g) + 1/2 O₂(g) K = 7.52 × 10-2 4 HCI(g) + O₂(g) = 2 Cl₂(g) + 2 H₂O(g) OK= 5.66 x 10-3 OK= 13.3 OK= 0.150 OK = 177 OK = 3.65 K = ?

The equilibrium constant (K1) for the reaction CO2 (g) 2 CO(g) +1/2 02(8) is 6.66 x 10-12 at 1000 K. Calculate K2 for the reaction 2 CO(g) + 02(g) 2 2002(g) K2 =

10. What is the expression for the equilibrium constant (K) for the reaction 2 C₂H(g) +7 O2(g) → 4 CO2(g) + 6 H₂O(g)? Tool Box: 1 cal 4.184 J 1Kcal 4.184 KJ 1000 cal 1 Kcal 1000 J = 1 KJ

Use the References to access important values if needed for this question. Consider the reaction: C(s) + 1/20₂(g) → CO(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: C(s) + O2(g) CO₂(g) K₁ CO(g) + 1/2O₂(g) = CO2 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K =

Phosgene is a chemical warfare agent first used on soldiers in World War I. It is synthesized according to the following gas-phase equilibrium reaction: CO(g) + Cl, (g) = COCI,(g) Write the equilibrium expression K, for this reaction below. K. = If K. = 0.281 for this reaction, would the product or the reactant be favored at equilibrium? The reactants would be favored. Neither the product nor the reactants would be favored. The product would be favored.