Question

1. At a given temperature the following equilibrium systems have the equilibrium constants shown below: S(s) + O2(g) ? SO2(g) Kc1= 4.2x10^52 2 S(s) + 3O2(g) ? 2SO3(g) Kc2= 9.8x10^128 Write the equilibrium expression for Kc3 as given by the equation below, and solve for Kc3 at 1123 K: SO2(g) + O2(g) ? SO3(g) Kc3 = ???? 2. Consider the following equilibrium systems and their corresponding equilibrium constants at 1123 K: C(s) + CO2(g) ? 2 CO(g) Kp1 = 1.3x10^14 CO(g) + Cl2(g) ? COCl2(g) Kp2= 6.0x10^-3 Write the equilibrium expression for Kp3, and solve for Kp3 at 1123 K for the overall reaction: C(s) + CO2(g) + 2Cl2(g) ? 2COCl2(g) Kp3 = ???? 3. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form COCl2(g) at 74 °C are [CO] = 0.012 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M. Calculate the equilibrium constants Kc and Kp. Consider R = 0.082 L atm K^-1 mol^-1 4. Consider the following equilibrium below at 295 k: NH4SH(S) ? HN3(g) + H2S(s) The partial pressure of each gas is 0.265 atm. Calculate Kp and Kc for the reaction. 

          1. At a given temperature the following equilibrium systems have the equilibrium constants shown below:

S(s) + O2(g) ? SO2(g) Kc1= 4.2x10^52
2 S(s) + 3O2(g) ? 2SO3(g) Kc2= 9.8x10^128

Write the equilibrium expression for Kc3 as given by the equation below, and solve for Kc3 at 1123 K:

SO2(g) + O2(g) ? SO3(g) Kc3 = ????

2. Consider the following equilibrium systems and their corresponding equilibrium constants at 1123 K:

C(s) + CO2(g) ? 2 CO(g) Kp1 = 1.3x10^14
CO(g) + Cl2(g) ? COCl2(g) Kp2= 6.0x10^-3

Write the equilibrium expression for Kp3, and solve for Kp3 at 1123 K for the overall reaction: C(s) + CO2(g) + 2Cl2(g) ? 2COCl2(g) Kp3 = ????

3. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form COCl2(g) at 74 °C are [CO] = 0.012 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M. Calculate the equilibrium constants Kc and Kp. Consider R = 0.082 L atm K^-1 mol^-1

4. Consider the following equilibrium below at 295 k:

NH4SH(S) ? HN3(g) + H2S(s)

The partial pressure of each gas is 0.265 atm. Calculate Kp and Kc for the reaction.
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1. At a given temperature the following equilibrium systems have the equilibrium constants shown below: S(s) + O2(g) ? SO2(g) Kc1= 4.2x10^52 2 S(s) + 3O2(g) ? 2SO3(g) Kc2= 9.8x10^128 Write the equilibrium expression for Kc3 as given by the equation below, and solve for Kc3 at 1123 K: SO2(g) + O2(g) ? SO3(g) Kc3 = ???? 2. Consider the following equilibrium systems and their corresponding equilibrium constants at 1123 K: C(s) + CO2(g) ? 2 CO(g) Kp1 = 1.3x10^14 CO(g) + Cl2(g) ? COCl2(g) Kp2= 6.0x10^-3 Write the equilibrium expression for Kp3, and solve for Kp3 at 1123 K for the overall reaction: C(s) + CO2(g) + 2Cl2(g) ? 2COCl2(g) Kp3 = ???? 3. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form COCl2(g) at 74 °C are [CO] = 0.012 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M. Calculate the equilibrium constants Kc and Kp. Consider R = 0.082 L atm K^-1 mol^-1 4. Consider the following equilibrium below at 295 k: NH4SH(S) ? HN3(g) + H2S(s) The partial pressure of each gas is 0.265 atm. Calculate Kp and Kc for the reaction.

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Chemistry: Structure and Properties
Chemistry: Structure and Properties
Nivaldo Tro 2nd Edition
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Transcript

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00:01 All right so we have equilibrium systems.
00:04 We're given questions on equilibrium systems.
00:10 The first one we're given the two equations and the corresponding k values and we have to write the equilibrium expression for another equation given those first two.
00:28 Now so the job here is to see you're going to apply some kind of hessian approach.
00:35 That's what we'll take where we're going to flip since the so2 is on the product reactant side in our equation.
00:43 We're going to flip the first equation which will mean that the k would be inverse.
00:48 The k value of the nu would be the inverse and that's what you can see right here and then for the second equation we're not going to flip.
00:55 We leave it because we want so3 on the right but we're going to divide the entire equation by two which will mean that we have to find the square root of the k.
01:05 That will change with it and then when you plug all of that in it means i can see the nu when you sum of that the nu put as the nu equilibrium constant sorry would be the first one the inverse of the first one multiplied by the square root of the second one and you would have this answer.
01:24 The same thing goes for this second question.
01:28 Right the first equation we will leave the way it is...
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