For each of the following reactions, indicate if the equilibrium mixture contains mostly products, mostly reactants, or both reactants and products:
a.
b.
c.
d.
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- Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%.arrow_forwardCarbon tetrachloride may react with oxygen to produce chlorine and carbonyl chloride. 2CCl4(g) + O2(g) ⇔ 2COCl2(g) + 2Cl2(g); Kc = 9.9 × 1051 What is Kc for the following equilibrium? COCl2(g) + Cl2(g)⇔ CCl4(g) + ½O2(g)arrow_forwardAt high temperatures nitrogen (N2) and oxygen (O2) will react to form NO.N2(g) + O2(g) ⇆ 2 NO(g) (4.1)The value for the equilibrium constant for reaction 4.1 is KC = 2.7 x 10^-17 at some temperature T.A system initially has [N2] = 0.0800 M and [O2] = 0.0500 M. There is no NO initially present inthe system. Find the value for [NO] that will be present at equilibrium.arrow_forward
- 7. 2CO2 (g) 200(g) + O2 (g). It was found that at 20 OC, the total pressure at equilibrium is 2.9 atm and that of CO2 is 0.8 atm. Calculate K. (Answer 2.14)arrow_forwardConsider the following system at equilibrium where AHⓇ 2SO2(g) + O2(g) = 2SO3 (9) When 0.24 moles of O₂ (g) are added to the equilibrium system at constant temperature: The value of K O increases decreases O remains the same The value of Qc O is greater than Kc O is equal to Kc O is less than Kc = 198 kJ, and Ke The concentration of SO2 will O increase decrease O remain the same The reaction must O run in the forward direction to reestablish equilibrium O run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium = 34.5, at 1150 K: Consider the following mat equilibrium where&ff-879 PC)+)-PC, ( Whe036PC (a) are added to the equum system at The K The Q Ogra Therearrow_forwardConsider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e)…arrow_forward
- 15.17 When the following reactions come to equilibrium, does the equilibrium mixture contain mostly reactants or mostly products? Kc = 1.5 × 10-10 (b) 2 SO2(8) + O2(8) = 2 S03(g) K,= 2.5 x 10° (a) N2(8) + O2(8) = 2 NO(g) %3Darrow_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_forwardNitrogen 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_forward
- 3.6arrow_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_forwardIn (6.7 At 600 °C, what is the value of the equilibrium constant for: C (s) + 2 PCI5 (g) = 2 PC|3 (g) + CCl4 (1) ? a. 1.3x10-⁹ b. 2.4x10-4 d. 1.9x105 c. 5.3x104 12. At 600 °C, the following reactions have these equilibrium constants: PC15 = PC|3 (g) + Cl2 (g) K = 6.77 x 10-5 (g) C(s) + 2 C/₂ (g) = CCl4 (1) K = 5.31 x 10+4 MOMOarrow_forward
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