A student ran the following reaction in the laboratory at 529 K: COC12 (9)CO(g) + Cl₂ (9) When she introduced 2.04 moles of COC1₂ (9) into a 1.00 liter container, she found the equilibrium concentration of COC12 (g) to be 2.00 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

For the reaction 2 H₂O(g) 2 H₂(g) + O₂(g) the equilibrium concentrations were found to be [H₂O] = 0.250 M, [H₂] = 0.420 M, and [0₂] = 0.750 M. What is the equilibrium constant for this reaction? Kc =

Consider the chemical reaction system represented by the following equation:

A student ran the following reaction in the laboratory at 288 K: 2CH₂Cl₂(9) CH4(9) + CCl4(9) When she introduced 7.50x 10-2 moles of CH₂Cl₂(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(9) to be 3.48x10-² M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

A student ran the following reaction in the laboratory at 545 K: COC12 (g) CO(g) + Cl₂ (g) When she introduced 0.604 moles of COC12 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂ (g) to be 0.0302 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

A sealed 3.5 L container initially holds 0.0127 moles of hydrogen gas, 0.084 moles of solid iodine, and 0.0581 moles of hydrogen iodide gas. When equilibrium is reached, the concentration of hydrogen is 0.0065 M. Calculate the value of the equilibrium constant, Keq, for the reaction H2(g)+I2(s)⟶2HI(g). For the equilibrium constant, use a 1.0 M standard state, not a 1.0 atm standard state. Keq= ?

Consider the following equilibria: 2SO3(g)    2SO2(g) + O2(g)                       Kc1 = 2.3 × 10 – 7 2NO3(g) ⟷   2NO2(g) + O2(g)                       Kc2 = 1.4 ×10 – 3 Calculate the equilibrium constant for the reaction: SO2(g) + NO3(g)   ⟷ SO3(g) + NO2(g) A 1.3 × 10 – 2 B 1.6 × 10 – 4 C 78 D 6.1 × 103

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 =

A student ran the following reaction in the laboratory at 655 K: 2NH3 (9) ⇒ N2 (g) + 3H2 (9) When she introduced 0.0871 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H₂(g) to be 0.119 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Кс

A student ran the following reaction in the laboratory at 1083 K: 2503(g) 2sO2(g) + 02(g) When she introduced 7.36x10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.23x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc II