Select the correct equilibrium expression for the reaction
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Chemistry
- Kp for the formation of phosgene, COCl2, is 6.5 1011 at 25 C. CO(g) + Cl2(g) COCl2(g) What is the value of Kp for the dissociation of phosgene? COCl2(g) CO(g) + Cl2(g)arrow_forwardHeating a metal carbonate leads to decomposition. BaCO3(s) BaO(s) + CO2(g) Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left or (iii) shifts right. (a) add BaCO3 (b) add CO2 (c) add BaO (d) raise the temperature (e) increase the volume of the flask containing the reactionarrow_forwardConsider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + |o2(g)^SO}(g) A, £ 2 SO,(g) «=* 2 SO,(g) + O,(g) A, Which of the following expressions relates A, to A2? A2 = A,2 A,2 = A, A2 = A, A2 = 1/A, A2 = 1/A,2arrow_forward
- For the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations are [SO2] = 0.102, [O2] = 0.0132, and [SO3] = 0.184. The concentration of SO2 is suddenly doubled. Show that the forward reaction takes place to reach a new equilibrium.arrow_forwardCalculate the value of the equilibrium constant Kp for the reaction 2NO2(g)+Cl2(g)2NOCl(g) from these equilibrium pressures: NO, 0.050 atm; Cl2, 0.30 arm; NOCI, 1.2 mm.arrow_forwardWhat is the value of the equilibrium constant at 500 C for the formation of NH3 according to the following equation? N2(g)+3H2(g)2NH3(g) An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 C was found to contain 1.35 M H2, 1.15 M N2, and 4.12101M NH3.arrow_forward
- The following reaction has an equilibrium constant Kc equal to 4.36 104 at 38C 2NOBr(g)2NO(g)+Br2(g) For each of the following compositions, decide whether the reaction mixture is at equilibrium. If it is not, decide which direction the reaction should go. a [NOBr] = 0.0720 M, [NO] = 0.0162 M, [Br2] = 0.0124 M b [NOBr] = 0 121 M, [NO] = 0.0159 M, [Br2] = 0.0139 M c [NOBr] = 0.103 M, [NO] = 0.0133 M, [Br2] = 0.0184 M d [NOBr] = 0.0472 M, [NO] = 0.0121 M, [Br2] = 0.0105 Marrow_forwardGiven the following descriptions of reversible reactions, write a balanced net ionic equation (simplest whole-number coefficients) and the equilibrium constant expression (K) for each. (a) Liquid acetone (C3H6O) is in equilibrium with its vapor. (b) Hydrogen gas reduces nitrogen dioxide gas to form ammonia and steam. (c) Hydrogen sulfide gas (H2S) bubbled into an aqueous solution of lead(ll) ions produces lead sulfide precipitate and hydrogen ions.arrow_forwardA necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?arrow_forward
- Ammonium hydrogen sulfide decomposes on heating. NH4HS(s) NH3(g) + H2S(g) If Kp for this reaction is 0.11 at 25 C (when the partial pressures are measured in atmospheres), what is the total pressure in the flask at equilibrium?arrow_forwardThe following reaction has an equilibrium constant Kc equal to 3.59 at 900C. CH4(g)+2H2S(g)CS2(g)+4H2(g) For each of the following compositions, decide whether the reaction mixture is at equilibrium. If it is not, decide which direction the reaction should go. a [CH4] = 1.26 M, [H2S] = 1.32 M, [CS2] = 1.43 M, [H2] = 1.12 M b [CH4] = 1.25 M, [H2S] = 1.52 M, [CS2] = 1.15 M, [H2] = 1.73 M c [CH4] = 1.30 M, [H2S] = 1.41 M, [CS2] = 1.10 M, [H2] = 1.20 M d [CH4] = 1.56 M, [H2S] = 1.43 M, [CS2] = 1.23 M, [H2] = 1.91 Marrow_forwardConsider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + 12 O2(g) SO3(g) K1 2SO3(g) 2SO2(g) + O2(g) K2 Which of the following expressions relates K1 to K2? (a) K2=K12 (b) K22=K1 (c) K2 = K1 (d) K2 = 1/K1 (e) K2=1/K12arrow_forward
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