The following reaction is at equilibrium at a pressure of 1 atm, in a closed container: C2H2(g) + 2H2(g) 5 C2H6(8); AHO =-311 kJ Which direction does the reaction shift when the volume of the container is increased? O toward reactants O toward products O no effect O cannot be determined

An equilibrium mixture contains 0.2500.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.2000.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container.   CO(g)+H2O(g)↽−−⇀CO2(g)+H2(g)CO(g)+H2O(g)⁢↽−−⇀⁢CO2⁢(g)+H2⁡(g)   How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.3000.300 mol once equilibrium has been reestablished? moles of CO2CO2 =

10) For the reaction: 2 V PC13(g) + Cl2(g) → PC15(g) at 85°C, Kp = 1.19 = If one starts with 2.00 atm pressure of PC13, 1.00 atm pressure of Cl2 and no PC15, what is the partial pressure of PC15(g) at equilibrium? A) 0.739 atm B) 0.621 atm C) 0.465 atm D) 0.167 atm E) 0.553 atm

Consider the equilibrium  2NO(g)⇌N2(g)+ O2(g) For which ΔH = -180kJ mol-1 how will adding H2(g) affect an equilibrium mixture of the three gases? a) Reaction will proceed to the left to generate more reaction b) reaction will proceed to the right to generate more product c) there will be no change to the equilibrium mixture

9) Given the following equilibrium reaction below, indicate which direction the reaction will shift when the indicated stresses are applied (à, ß, or none), AND indicate how the K value will change (increase, decrease or stays same) with the stress. P = 1 atm, unless otherwise specified. ​​CO(g) + Cl2(g) ó COCl2(g) ​ H = –107.6 kJ/mol What will happen if:​​​​​Shift​​​K value i) The pressure is quadrupled​​​​_______​_________________​ ii) The reaction temperature is decreased​​_______​__________________ iii) More COCl2 gas is added​​​​_______​__________________ iv) The volume is doubled​​​​_______​__________________

Equilibrium: 7. Write the equilibrium expression, K, for the following reactions: 2NH, (g) + CO2 (g) N,CH,0 (s) + H,0 (g) K= N2 (g) + 02 (g) 2 NO (g) K= 8. Consider the following reaction at equilibrium. 2S0, (g) 2S0, (g) + 02 (g) Predict the affect on equilibrium (will it shift left, shift right or no change?): a. Oxygen gas is removed: b. The volume is increased: c. The pressure is increased: d. SO, is added: e. SO, is added:

The reaction A 2 + B 2 =2 AB has an equilibrium constant Kc = 64. The following pictures represent reaction mixtures that contain A 2 molecules (shaded) and B 2 molecules (unshaded), and AB molecules. Which reaction mixture is at equilibrium? 00 (1) (2) (4) reaction mixture (1) reaction mixture (2) reaction mixture (3) reaction mixture (4) O000

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Consider the equilibrium  2NO(g)⇌N2(g)+ O2(g) For which ΔH = -180kJ mol-1 how will adding Xe(g) affect an equilibrium mixture of the three gases? a) Reactioj will proceed to the left to generate more reaction b) reaction will proceed to the right to generate more product c) there will be no change to the equilibrium mixture