MISSED THIS? Read Section 16.6 (Pages 696 - 699). Consider the following reaction: Part A CO (g) + 2 H2 (g) = CH3OH (g) An equilibrium mixture of this reaction at a certain temperature was found to have CO = 0.115 M, H2] = 0.118 M, and [CHОН- 0.190 М. What is the value of the equilibrium constant (K.) at this temperature? Express your answer numerically to three significant figures. > View Available Hint(s) Πνα ΑΣφ K. = Submit

3. Initially 2.25 mol of carbon monoxide gas, CO) and 2.25 mol of water vapour, H₂O(g), are placed in a 1.50 L container and equilibrium is established and Keq is 4.2. Determine all equilibrium concentrations. CO (6) + H₂O (8) [02]}} + H₂

At a certain temperature, the following reactions have the equilibrium constants shown. S(s) + O2(g) ⇆ SO2(g).  Kc1 = 4.2 × 1052 2S(s) + 3O2(g) ⇆ 2SO3(g).  Kc2 = 9.8 × 10128 Calculate the equilibrium constant, Kc, for the following reaction at that temperature. (in scientic notation) 2SO2(g) + O2(g) ⇆ 2SO3(g)

Consider the reaction;  N2(g) + O2(g)⇆ 2 NO(g)  where K = 0.10.      Starting with initial concentrations of [N2] = 0.04 M and [O2] = 0.40 M,      the equilibrium concentration of NO is

Kc=?

2 CO₂ (g) = 2 CO (g) + O₂ (g) 1. Write the K. expression for this balanced equation. 2. If, at equilibrium, the concentrations of the reactants and products are as follows: [CO] = 0.00025 M, [0₂] = 0.00050, [CO₂] = 0.25 M, calculate the value for Kc. 3. Where does the equilibrium lie, towards the products or reactants? How can you know?

The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.

At 773 °C, a mixture of CO(g), H2(g), and CH3OH(g) was allowed to come to equilibrium. The concentrations were determined to be: [CO] = 0.105 M, [H2] = 0.250 M, [CH3OH] = 0.00261 M. Calculate K. for the reaction CO(g) + 2H2(g) CH3OH(g) Kc = %3D

A student ran the following reaction in the laboratory at 282 K: 2CH2C12(g)=CH4(g)+ CCI4(g) When she introduced 6.98x102 moles of CH,Ch(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62x10³ M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =

n9 of 21 At 379 K, this reaction has a K. value of 0.0581. X(g) +3 Y(g) 2 Z(g) Calculate K, at 379 K. Note that the pressure is in units of atmosphere (atm). Kp =