3. Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium: a. A 1.00 L flask containing 0.0500 mol NO (g), 0.0155 mol Cl₂ (g), and 0.500 mol NOCI(g): 2NO(g) + Cl₂(g) = 2NOCI(g) = 4.6 × 10¹ A: shift right Keq b. A 5.00 L flask containing 14 g N₂ (g), 12 g H₂ (g), and 17 g NH3(g): N₂(g) + 3H₂(g) = 2NH3(g) Keq = 0.060 (at 526 °C) c. A 2.00 L flask containing 230 g SO3 (8) 2SO3(8)2SO₂(g) + O₂(g) Keg = 0.230 A: shift left A: shift right

Consider the following reaction where Kc = 154 at 298 K. 2NO(g) + Br₂(g) —2NOBr(g) A reaction mixture was found to contain 2.48×10-2 moles of NO(g), 3.91×10-2 moles of Br₂(g) and 8.22x10-2 moles of NOBr(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium. Submit Answer Retry Entire Group 9 more group attempts remaining

Phosphorus pentachloride decomposes at higher temperatures. PC15(g) → PCl3(g) + Cl₂(g) Z An equilibrium mixture at some temperature consists of 5.77 g PCL5, 208.23 g/mol 4.86 g PC|3, 137.33 g/mol 3.59 g Cl₂, 70.91 g/mol in a 1.00-L flask. If you add 1.31 g of Cl₂, how will the equilibrium be affected and what will the concentration of PCI5 be when equilibrium is reestablished? shift left shift right no shift will occur [PCI5] = 0.0276 mol/L

Given K, and all but one of the equilibrium concentrations, find the concentration of the one that was not given. Example:                    Z2   D     2 Z An equilibrium mixture of Z2 and Z has [Z] = 0.93 M.  Find [Z2], given that the value of K is 5.00.        Given K and the initial concentrations of all reactants and products, find the final (equilibrium) concentrations.  Example:                     Z2        D            2 Z   initial concs:               0.400M            0.000M   Given K and the concentrations of all reactants and products, determine if the reaction is at equilibrium. If it is not, determine which way the reaction will go.  In the hardest version of this problem type, determine the equilibrium concentrations.  Example:  Is the system below at equilibrium? (K is equal to 5.00.)   If not, which way will the reaction go?  Find the equilibrium concentrations.                                     Z2        D            2 Z concs:              2.00 M…

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Consider the following reaction:   SO2Cl2(g)⇌SO2(g)+Cl2(g)SO2Cl2(g)⇌SO2(g)+Cl2(g)   A reaction mixture is made containing an initial [SO2Cl2][SO2Cl2] of 2.3×10−2 MM . At equilibrium, [Cl2]=[Cl2]= 1.2×10−2 MM .   Calculate the value of the equilibrium constant (Kc)(Kc).   Express your answer to two significant figures.

For the reaction at equilibrium: 2 H2O (g) +2 Cl 2 (g) + energy4 HCI (g) + O2 (g), If the temperature in the reaction vessel is decreased: O [H2O] will decrease. [H2O] will increase. [H2O] will not change.

NAME: COC12(g) has a 8. At 100.0°C, the equilibrium constant for the reaction: COg) + Cl2(g) value of 4.6 x 10°, If 0.40 mol of COC12 is placed into a 10.0 L flask at 100.0°C, what will be the equilibrium concentration of all species? (A simplifying approximation that will make the solution of the resulting equation easier is to note that X is much less than 0.040 mol/L. This means that 0.040-x is approximately 0.040.)

1. In your own words, explain the difference between the equilibrium constant, K, and the reaction quotient, Q. How do we use K and Q to determine what will happen to a specific reaction under a given set of conditions?

Consider the reaction. Br2(g)+Cl2(g)⇌2BrCl(g) Kp=1.11×10−4 at 150 K A reaction mixture initially contains a Br2 partial pressure of 755 torr and a Cl2 partial pressure of 735 torr at 150 K. Calculate the equilibrium partial pressure of BrCl.