1) At 453 °C, Keq is 1.33 for the following reaction: A(s) + 2B(g) ⇄C(s) +...
1) At 453 °C, Keq is 1.33 for the following reaction:
A(s) + 2B(g) ⇄C(s) + D(g)
If B gas at 0.793 bar is injected into a container at 453 °C that contains excess A, what are the partial pressures of all gases present at equilibrium?
a) Pressure of B
b) Pressure of D
Homework Answers
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1) At 453 °C, Keq is 1.33 for the following
reaction:
A(s) + 2B(g) ⇄C(s) +...
Chapter 14, Question 37 Parameterization At 412 °C, Kn is 0.502 for the following reaction: 2A(s) B(g)C(s) 2D(g) If B g...
Chapter 14, Question 37 Parameterization At 412 °C, Kn is 0.502 for the following reaction: 2A(s) B(g)C(s) 2D(g) If B gas at 1.02 bar is injected into a container at 412 °C that contains excess A, what are the partial pressures of all gases present at equilibrium? a) Pressure of B bar the tolerance is +/-2% LINK TO TEXT b) Pressure of D bar the tolerance is +/-2% LINK TΟΤΕXΤ
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400...
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
Consider the reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for each value...
Consider the reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for each value of K. Assume that the initial partial pressure of B in each case is 1.0 bar and that the initial partial pressure of Ais 0.0 bar. Make any appropriate simplifying assumptions. b）K= 1.1×10−4 Pa,Pb= ______bar c)K= 2.1×105 Pa,Pb= ______bar
1) At 100 oC, Keq = 1.5E8 for the reaction: CO(g) + Cl2(g) COCl2(g) Using appropriate...
1) At 100 oC, Keq = 1.5E8 for the
reaction:
CO(g) + Cl2(g)
COCl2(g)
Using appropriate approximation, calculate the partial pressure
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initially contains COCl2 at a pressure of 0.293 bar.
Consider the system at 25.0°C A(g) + 2B(g) + C(g) 2D(g) At time zero, only A,...
Consider the system at 25.0°C A(g) + 2B(g) + C(g) 2D(g) At time zero, only A, B and C are present in a sealed container. The reaction reaches equilibrium 10 minutes after the reaction is initiated. The partial pressures of A, B, C and D are written as Pa, PB, Pc and PD. Pc at 10 min is Pc at 9 min. v Po at 11 min is Po at 12 min. Select Greater than More information required Equal to...
Ammonium iodide, a solid, decomposes to give NH3(g) and HI(g). At 406 °C, some NH4I(s) is...
Ammonium iodide, a solid, decomposes to give NH3(g) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.08 atm. Extra NH3(g) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(g) is 1.27 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. NH4I(s) -->NH3(g) + HI(g) K...
At 100 oC, Keq = 1.5E8 for the reaction: CO(g) + Cl2(g) COCl2(g) Using appropriate approximation, calculate...
At 100 oC, Keq = 1.5E8 for the reaction: CO(g) + Cl2(g) COCl2(g) Using appropriate approximation, calculate the partial pressure of CO at 100 oC at equilibrium in a chamber that initially contains COCl2 at a pressure of 0.260 bar. bar The number of significant digits is set to 2; the tolerance is +/-4%
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and Bfor each of...
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and Bfor each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. A.)Kp= 2.0 B.) Kp= 1.6×10−4 C.)Kp= 1.4×105
Consider the reaction A(g) + 2B(g) ⇌ C(g) at 25 °C. The initial pressures of all...
Consider the reaction A(g) + 2B(g) ⇌ C(g) at 25 °C. The initial pressures of all the gases are 0.100 atm. Once equilibrium has been established, it is found that Pc = 0.140 atm. What is Kp for this reaction at 25 °C. Please explain and/or show the steps.
For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35...
For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35 x 10^4. Hydrogen at a partial pressure of 0.700 bar and chlorine at a partial pressure of 0.500 bar are placed in a vessel at 800oC and allowed to equilibrate. Find the final partial pressures of all three gases in this reaction in bar
Chapter 14, Question 37 Parameterization At 412 °C, Kn is 0.502 for the following reaction: 2A(s) B(g)C(s) 2D(g) If B gas at 1.02 bar is injected into a container at 412 °C that contains excess A, what are the partial pressures of all gases present at equilibrium? a) Pressure of B bar the tolerance is +/-2% LINK TO TEXT b) Pressure of D bar the tolerance is +/-2% LINK TΟΤΕXΤ
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
Consider the system at 25.0°C A(g) + 2B(g) + C(g) 2D(g) At time zero, only A, B and C are present in a sealed container. The reaction reaches equilibrium 10 minutes after the reaction is initiated. The partial pressures of A, B, C and D are written as Pa, PB, Pc and PD. Pc at 10 min is Pc at 9 min. v Po at 11 min is Po at 12 min. Select Greater than More information required Equal to...
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