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3. For the dissociation of gaseous PCls, the value of K, 2.00. The equilibrium reaction is...
At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) <=> 2BrCl...
At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) <=> 2BrCl (g) is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 atm of BrCl (g). What is the equilibrium pressure of Br2? A. 0.86 atm B. The equilibrium partial pressures of Br2 will be the same as the initial value. C. The equilibrium partial pressure of Br2 will be...
23) At 400 K, the equilibrium constant for the reaction Br2(g) + Cl2 (9) 2BrCl (9)...
23) At 400 K, the equilibrium constant for the reaction Br2(g) + Cl2 (9) 2BrCl (9) is Kp = 70. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g) 1.00 atm of Cl2 (g), and 2.00 alm of BrCl (g). Use Q to determine which of the statements below is true. A) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. B) The equilibrium partial pressures of Br2....
At 400 K, the equilibrium constant for the reaction Br 2 (g) + Cl 2 (g) 2BrCl...
At 400 K, the equilibrium constant for the reaction Br 2 (g) + Cl 2 (g) 2BrCl (g) is K p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br 2 (g), 1.00 atm of Cl 2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true. The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. The reaction will...
10. Using the equation shown below, calculate the equilibrium concentration of each species in a mixture...
10. Using the equation shown below, calculate the equilibrium concentration of each species in a mixture containing 0.0500 M PCls and 5,00 M PCI K for this reaction is 3.33 x 10' at 487 °C. PCs () PC:(8) + Cl() Suvishortliwabidi a llo 11. At equilibrium, the partial pressures of NO2, NO, and O, were found to be 0.200 atm, 0.00026 atm, and 0.600 atm, respectively, in a 1-liter flask. 2NO, (g) 2NO(g) + O2(g) s obomb (a) Write the...
At 283 K and a total equilibrium pressure of 0.989 atm, the fractional dissociation of NO...
At 283 K and a total equilibrium pressure of 0.989 atm, the fractional dissociation of NO is 0.363 for the reaction 2NO(g)N2(g) + 02(g) This means that 363 of every 1000 molecules of NO originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp. Kp
At 283 K and a total equilibrium pressure of 0.989 atm, the fractional dissociation of NO is 0.363 for the reaction 2NO(g)N2(g) + 02(g) This means that 363 of every 1000 molecules...
please show all work thanks B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter...
please show all work
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B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter flask at 25°C. When equilibrium at that temperature, it was determined that the ammonia was reduced A 2.568-g sample was reached N to 75.0% of its original value. 1. Calculate K for the decomposition of 2.00 moles of ammonia at 25.0°C. 2. Calculate K for the decomposition of 2.00 moles of ammonia at NH3 is...
At 25°C, the equilibrium constant K for the reaction in the solven 2BrCl = Br2 +...
At 25°C, the equilibrium constant K for the reaction in the solven 2BrCl = Br2 + Cl2 is 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine? 1.35 x 10-3M 2.70 x 10-3M 8.82 x 10-3 M 9.70 x 10-2 M. none of these choices is correct Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. D. NH4Is) + NH3(g) +HI(g) At 400°C, Kp =...
Answer the questions about the following reaction below. The equilibrium constant for the decomposition of PCls...
Answer the questions about the following reaction below. The equilibrium constant for the decomposition of PCls at 250°C is 0.041 ΔH is positive; reactants and products are gases at 250°C. Refer to your textbook. 1. Is the reaction above exothermic or endothermic? 2. What happens to the concentrations of PCls and Cl if more PCls is added once the reaction reaches equilibrium? (increases, decreases) PC1s Cl2 3. What happens to the moles of PCIs, PCls and Cl in the container...
1. The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <---->...
1. The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <----> PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.00 atm at 500 K. PPCl5 = atm PPCl3 = atm PCl2 = atm 2. The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K: NH4I(s) <----> NH3(g) + HI(g) Calculate the equilibrium partial pressure of HI when...
The equilibrium constant in terms of pressures for the reaction COCl2(g) <--> CO(g) + Cl2(g) is...
The equilibrium constant in terms of pressures for the reaction COCl2(g) <--> CO(g) + Cl2(g) is Kp = 5.00 at 873 K. (a) A pure sample of gaseous phosgene, COCl2(g), is introduced into a rigid flask at a temperature of 873 K so that its original pressure is 0.121 atm. Calculate the fraction of this starting material that is converted to products at equilibrium. (b) A second sample of phosgene is introduced into a rigid flask at a temperature of...
23) At 400 K, the equilibrium constant for the reaction Br2(g) + Cl2 (9) 2BrCl (9) is Kp = 70. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g) 1.00 atm of Cl2 (g), and 2.00 alm of BrCl (g). Use Q to determine which of the statements below is true. A) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. B) The equilibrium partial pressures of Br2....
10. Using the equation shown below, calculate the equilibrium concentration of each species in a mixture containing 0.0500 M PCls and 5,00 M PCI K for this reaction is 3.33 x 10' at 487 °C. PCs () PC:(8) + Cl() Suvishortliwabidi a llo 11. At equilibrium, the partial pressures of NO2, NO, and O, were found to be 0.200 atm, 0.00026 atm, and 0.600 atm, respectively, in a 1-liter flask. 2NO, (g) 2NO(g) + O2(g) s obomb (a) Write the...
At 283 K and a total equilibrium pressure of 0.989 atm, the fractional dissociation of NO is 0.363 for the reaction 2NO(g)N2(g) + 02(g) This means that 363 of every 1000 molecules of NO originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp. Kp
At 283 K and a total equilibrium pressure of 0.989 atm, the fractional dissociation of NO is 0.363 for the reaction 2NO(g)N2(g) + 02(g) This means that 363 of every 1000 molecules...
please show all work
thanks
B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter flask at 25°C. When equilibrium at that temperature, it was determined that the ammonia was reduced A 2.568-g sample was reached N to 75.0% of its original value. 1. Calculate K for the decomposition of 2.00 moles of ammonia at 25.0°C. 2. Calculate K for the decomposition of 2.00 moles of ammonia at NH3 is...
At 25°C, the equilibrium constant K for the reaction in the solven 2BrCl = Br2 + Cl2 is 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine? 1.35 x 10-3M 2.70 x 10-3M 8.82 x 10-3 M 9.70 x 10-2 M. none of these choices is correct Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. D. NH4Is) + NH3(g) +HI(g) At 400°C, Kp =...
Answer the questions about the following reaction below. The equilibrium constant for the decomposition of PCls at 250°C is 0.041 ΔH is positive; reactants and products are gases at 250°C. Refer to your textbook. 1. Is the reaction above exothermic or endothermic? 2. What happens to the concentrations of PCls and Cl if more PCls is added once the reaction reaches equilibrium? (increases, decreases) PC1s Cl2 3. What happens to the moles of PCIs, PCls and Cl in the container...
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