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128 HW 13 14.41 For the reaction the equilibrium constant K. at 375°C is 1.2. Starting with [H,lo 0.76 M, [N2lo 0.60 M, and [NH,lo 0.48 M, which gases will have increased in concen- tration and which will have decreased in concentra- tion when the mixture comes to equilibrium? H2(g) + CO2(g) H,0(g) + CO(g) at 700°C, K.= 0.534. Calculate the number of moles of H, that are present at equilibrium if a mix- ture of 0.300 mole of CO and 0.300 mole of H,0 is %3D heated to 700°C in a 10.0-L container. 14.42 At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) = 2NO(g) + O2(g) The equilibrium constant Kp is 158. Analysis shows that the partial pressure of O2, is 0.25 atm at equilibrium. Calculate the pressure of NO and NO, in the mixture. HW13 14.43 The equilibrium constant K. for the reaction H2(g) + Br2(g) = 2HB1(g) is 2.18 × 10° at 730°C. Starting with 3.20 moles of HWT5 HBr in a 12.0-L reaction vessel, calculate the con- centrations of H2, Br2, and HBr at equilibrium. 14.44) The dissociation of molecular iodine into iodine at- oms is represented as L(g) = 21(g) At 1000 K, the equilibrium constant K. for the -5 reaction is 3.80 x 10. Suppose you start with 0.0456 mole afL in a 2.30-L flask at 1000 K. What are the concenrations of the gases at equilibrium? 0.00 14.45 The equilibrium constant K. for the decomposition of phosgene, COCI, is 4.63 × 10-³ at 527°C: COC, (8) = CO(g) + Cl2(8) quilibrium partial pressure of all the at 0.760 atm ene

128 HW 13 14.41 For the reaction the equilibrium constant K. at 375°C is 1.2. Starting with [H,lo 0.76 M, [N2lo 0.60 M, and [NH,lo 0.48 M, which gases will have increased in concen- tration and which will have decreased in concentra- tion when the mixture comes to equilibrium? H2(g) + CO2(g) H,0(g) + CO(g) at 700°C, K.= 0.534. Calculate the number of moles of H, that are present at equilibrium if a mix- ture of 0.300 mole of CO and 0.300 mole of H,0 is %3D heated to 700°C in a 10.0-L container. 14.42 At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) = 2NO(g) + O2(g) The equilibrium constant Kp is 158. Analysis shows that the partial pressure of O2, is 0.25 atm at equilibrium. Calculate the pressure of NO and NO, in the mixture. HW13 14.43 The equilibrium constant K. for the reaction H2(g) + Br2(g) = 2HB1(g) is 2.18 × 10° at 730°C. Starting with 3.20 moles of HWT5 HBr in a 12.0-L reaction vessel, calculate the con- centrations of H2, Br2, and HBr at equilibrium. 14.44) The dissociation of molecular iodine into iodine at- oms is represented as L(g) = 21(g) At 1000 K, the equilibrium constant K. for the -5 reaction is 3.80 x 10. Suppose you start with 0.0456 mole afL in a 2.30-L flask at 1000 K. What are the concenrations of the gases at equilibrium? 0.00 14.45 The equilibrium constant K. for the decomposition of phosgene, COCI, is 4.63 × 10-³ at 527°C: COC, (8) = CO(g) + Cl2(8) quilibrium partial pressure of all the at 0.760 atm ene

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128 HW 13 14.41 For the reaction the equilibrium constant K. at 375°C is 1.2. Starting with [H,lo 0.76 M, [N2lo 0.60 M, and [NH,lo 0.48 M, which gases will have increased in concen- tration and which will have decreased in concentra- tion when the mixture comes to equilibrium? H2(g) + CO2(g) H,0(g) + CO(g) at 700°C, K.= 0.534. Calculate the number of moles of H, that are present at equilibrium if a mix- ture of 0.300 mole of CO and 0.300 mole of H,0 is %3D heated to 700°C in a 10.0-L container. 14.42 At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) = 2NO(g) + O2(g) The equilibrium constant Kp is 158. Analysis shows that the partial pressure of O2, is 0.25 atm at equilibrium. Calculate the pressure of NO and NO, in the mixture. HW13 14.43 The equilibrium constant K. for the reaction H2(g) + Br2(g) = 2HB1(g) is 2.18 × 10° at 730°C. Starting with 3.20 moles of HWT5 HBr in a 12.0-L reaction vessel, calculate the con- centrations of H2, Br2, and HBr at equilibrium. 14.44) The dissociation of molecular iodine into iodine at- oms is represented as L(g) = 21(g) At 1000 K, the equilibrium constant K. for the -5 reaction is 3.80 x 10. Suppose you start with 0.0456 mole afL in a 2.30-L flask at 1000 K. What are the concenrations of the gases at equilibrium? 0.00 14.45 The equilibrium constant K. for the decomposition of phosgene, COCI, is 4.63 × 10-³ at 527°C: COC, (8) = CO(g) + Cl2(8) quilibrium partial pressure of all the at 0.760 atm ene
Transcribed Image Text:128 HW 13 14.41 For the reaction the equilibrium constant K. at 375°C is 1.2. Starting with [H,lo 0.76 M, [N2lo 0.60 M, and [NH,lo 0.48 M, which gases will have increased in concen- tration and which will have decreased in concentra- tion when the mixture comes to equilibrium? H2(g) + CO2(g) H,0(g) + CO(g) at 700°C, K.= 0.534. Calculate the number of moles of H, that are present at equilibrium if a mix- ture of 0.300 mole of CO and 0.300 mole of H,0 is %3D heated to 700°C in a 10.0-L container. 14.42 At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) = 2NO(g) + O2(g) The equilibrium constant Kp is 158. Analysis shows that the partial pressure of O2, is 0.25 atm at equilibrium. Calculate the pressure of NO and NO, in the mixture. HW13 14.43 The equilibrium constant K. for the reaction H2(g) + Br2(g) = 2HB1(g) is 2.18 × 10° at 730°C. Starting with 3.20 moles of HWT5 HBr in a 12.0-L reaction vessel, calculate the con- centrations of H2, Br2, and HBr at equilibrium. 14.44) The dissociation of molecular iodine into iodine at- oms is represented as L(g) = 21(g) At 1000 K, the equilibrium constant K. for the -5 reaction is 3.80 x 10. Suppose you start with 0.0456 mole afL in a 2.30-L flask at 1000 K. What are the concenrations of the gases at equilibrium? 0.00 14.45 The equilibrium constant K. for the decomposition of phosgene, COCI, is 4.63 × 10-³ at 527°C: COC, (8) = CO(g) + Cl2(8) quilibrium partial pressure of all the at 0.760 atm ene
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