The numerical value of the equilibrium constant,
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- 1:18 Question 1 of 16 Consider the following chemical reaction at equilibrium: 2NO₂(g) = N₂O4(9) A) reactants If the container's volume is increased by a factor of 2, in which direction will the equilibrium shift? B) product Submit C) neither the reactants nor the product Tap here or pull up for additional resourcesarrow_forwardConsider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.arrow_forwardConsider the endothermic reactionC (s) + H2O (g) ⇄ CO (g) + H2 (g)If the system is allowed to reach equilibrium, which direction will it shift if the following stresses are applied? (11a) Increase volume (11b) Decrease temperaturearrow_forward
- (#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.arrow_forward7 4 (a) Calculate the value of Kc for the reaction: PC15 (2) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PCls (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCls (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (1) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalystarrow_forward(10b) The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600K. COCl2(g) CO(g) + Cl2(g)If an equilibrium mixture of the three gases in a 11.8 L container at 600K contains 0.303 mol of COCl2(g) and 0.320 mol of CO, the equilibrium concentration of Cl2 is M. (25a) The equilibrium constant, K, for the following reaction is 1.75×10-2 at 609 K.COCl2 (g) CO (g) + Cl2 (g) An equilibrium mixture of the three gases in a 14.0 L container at 609 K contains 0.209 M COCl2, 6.04×10-2 M CO and 6.04×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 5.82 L? [COCl2] = M [CO] = M [Cl2] = Marrow_forward
- 9 At a certain temperature, 1.00 mole sulfur trioxide (SO3) is introduced into a 1.00 L container. The SO3 partially dissociates by the reaction: + O2 (g) 2 SO3(g) 2 SO₂ If 0.300 moles O₂ is present at equilibrium, what is the value of ke for this reaction? Your answer, 1.91, is incorrect by more than 10%.arrow_forward4:15 Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 1.25 L flask at 25.0 °C. The flask is found to contain 2.35 g of NO2, 9.60 g of N₂O, and 4.50 g of O₂. What is the value of Kc for this reaction? 4 NO₂(g) 2 N₂O(g) + 3 O₂(g) Question 8 of 10 Kc = Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [0.0409]² [0.218] [0.113] ³ [0.0409]¹ 0.480 Once the expression is constructed, solve for Kc. 3.57 x 10³ 1 [0.175]² [0.141] [0.0409] [0.175]4 0.0642 Submit [0.113]² [0.0409]³ [0.175] [0.113]4 28.7 Tap here or pull up for additional resources RESET [0.0511] [0.175]³ [0.113] 15.8 13.6arrow_forwardPlease show all your work, including your ICE table for the following question.arrow_forward
- Nitrogen dioxide dimerizes according to the following reaction: 2 NO₂ (9) K₂ = 6.7 at 298 K N₂O4 (9) A 2.25-L container contains 0.055 mol of NO₂ and 0.082 mol of N₂O4 at 298 K. Part A Is the reaction at equilibrium? If not, in what direction will the reaction proceed? The reaction is at equilibrium. The reaction is not at equilibrium and will shift to the left. The reaction is not at equilibrium and will shift to the right.arrow_forward302(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 Oarrow_forwardPhosgene COCl2, one of the gases used in chemical warfare in World War I, is produced by this simple exothermic reaction. Co (g) + Cl2 (9) COC2 (g) Phosgene What effect (increase, decrease, remain the same) does each of the following operations have on the amount of phosgene present at equilibrium? a.) Adding more Cl2 at constant volume b.) Lowering the temperature c.) Removing CO d.) Adding a catalyst e.) Decreasing the volume of the containerarrow_forward
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