Which change causes the equilibrium to shift to the product side? 2 CO) + O2(2) 2 CO2(2) AH= - (3)0) 283.3kJ (3)2) (3)2) ORemoving oxygen O Increasing the temperature O Adding carbon dioxide Removing carbon monoxide Decreasing the volume

The reaction A2 + B2 =2 AB has an equilibrium constant Kc = 9.0. The following pictures represent reaction mixtures that contain A2 molecules (shaded) and B2 molecules (unshaded), and AB molecules. Which reaction mixture is at equilibrium? 0 618 ∞ 8 00 (1) (2) (4) reaction mixture (1) reaction mixture (2) reaction mixture (3) reaction mixture (4) O O O O

At a certain temperature, the equilibrium constant K for the following reaction is 734.: NO3(g) + NO(g) 2 NO₂(g) Use this information to complete the following table. ?

Use arrows (up / down) to indicate the affect of each of these disturbances (stresses) on the concentration of the reactants and products in this equilibrium: 9 KJ + 2 S02 9) + 02 (9) = 2 S03 (9A disturbance affect on affect on affect on ISO2] [02] ISO3] decrease [SO2] increase [02] increase [SO3] increase pressure decrease temp Period 4 CHE

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(#30) The Equilibrium Constant and the "ICE Chart" Phosphorus pentachloride gas is formed according to the reaction by adding chlorine gas to phosphorus trichloride gas. Then the reaction reaches equilibrium. The equilibrium constant, Kc, equals 49.0 at 230°C. If 0.500 mole each of the reactants are added to a 5-L container, what is the equilibrium composition at 230°C? (30a) In blank #1, type-in our answer for the concentration of phosphorus pentachloride in the product at equilibrium. The unit is Molarity, but enter only the value of your answer with two decimal places. (30b) In blank #2, type in your answer for the concentration of phosphorus trichloride at equilibrium with two decimal places. (30c) In blank #3, type in your answer for the concentration of chlorine gas at equilibrium with two decimal places.

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204(g) = 2NO2(g) A 1.000-L flask is charged with 0.0300 mol of N204. At equilibrium, 0.0204 mol of N204 remains. Calculate the Kc for this reaction. (Enter only the numerical value to three significant figures without units.) Answer:

For the following reaction, calculate all equilibrium concentrations if  you start with 1.6 moles of nitrogen                  dioxide gas in a 4.0 L container.         2NO2(g) <====>  N2O4(g)            Keq = 1.5 at  250C

(Q96) The equilibrium constant with respect to concentration (K) fer the reaction between nitrogen monoxide and oxygen gas to produce nitrogen diexide is 5.4 x 1013 at 25 C. What is the value ef the equilibrium constant with respect to partial pressures (Ke) under these same eenditiens? (2 sf) O 2.2 x 10^12 O5.4 x 10A13 1.3 x 19A15 @ 11x 1014 2.2x10 10

302(9) = 203(g) O decreasing the volume will shift equilibrium in the direction of products O decreasing the volume will shift equilibrium in the direction of reactants no shift occurs Submit Request Answer Part B (6)o + (6)007 = (6)z007 decreasing the volume will shift equilibrium in the direction of products decreasing the volume will shift equilibrium in the direction of reactants no shift occurs Reguest Answer Submit Part C P.(g) + 50,(g) = P,010 (4) O decreasing the volume will shift equilibrium in the direction of products O decreasing the volume will shift alibrium in the direction of reactants no shift occurs Submit Reguest Answer Part D 2s0,(9) + 2H,0(g) = 2H,S(g) + 30,(g) O decreasing the volume will shift equilibrium in the direction of products decreasing the volume will shift equilibrium in the direction of reactants O no shift occurs O O