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2) A + B ? AB K1 = [AB] / ([A][B]) = 4.0 AB + D ? E + A K2 = ([E][A]) / ([AB][D]) = 3.0 B + D ? E K3 = [E] / ([B][D]) = 12 Given the equations above, how were equations 1 & 2 manipulated to create equation 3? 3) Consider reactions A and B at a particular temperature: Reaction A: NiO(s) + H2(g) ? Ni(s) + H2O(g) Kp = 50 Reaction B: NiO(s) + CO(g) ? Ni(s) + CO2(g) Kp = 700 Reaction C: CO2(g) + H2(g) ? CO(g) + H2O(g) Kp = ? Calculate the Kp value for Reaction C at this temperature. 4) The formation of a complex ion occurs in several steps. Given the series of steps and equilibrium constants below, calculate the equilibrium constant for: A3+(aq) + 2NH2-(aq) ? A(NH2)2+(aq) A3+(aq) + NH2-(aq) ? ANH2^2+(aq) K1 = 200 ANH2^2+(aq) + NH2-(aq) ? A(NH2)2+(aq) K2 = 125 

          2) A + B ? AB K1 = [AB] / ([A][B]) = 4.0
AB + D ? E + A K2 = ([E][A]) / ([AB][D]) = 3.0
B + D ? E K3 = [E] / ([B][D]) = 12
Given the equations above, how were equations 1 & 2 manipulated to create equation 3?

3) Consider reactions A and B at a particular temperature:
Reaction A: NiO(s) + H2(g) ? Ni(s) + H2O(g) Kp = 50
Reaction B: NiO(s) + CO(g) ? Ni(s) + CO2(g) Kp = 700
Reaction C: CO2(g) + H2(g) ? CO(g) + H2O(g) Kp = ?
Calculate the Kp value for Reaction C at this temperature.

4) The formation of a complex ion occurs in several steps. Given the series of steps and equilibrium constants below, calculate the equilibrium constant for: A3+(aq) + 2NH2-(aq) ? A(NH2)2+(aq)
A3+(aq) + NH2-(aq) ? ANH2^2+(aq) K1 = 200
ANH2^2+(aq) + NH2-(aq) ? A(NH2)2+(aq) K2 = 125
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2) A + B ? AB K1 = [AB] / ([A][B]) = 4.0 AB + D ? E + A K2 = ([E][A]) / ([AB][D]) = 3.0 B + D ? E K3 = [E] / ([B][D]) = 12 Given the equations above, how were equations 1 2 manipulated to create equation 3? 3) Consider reactions A and B at a particular temperature: Reaction A: NiO(s) + H2(g) ? Ni(s) + H2O(g) Kp = 50 Reaction B: NiO(s) + CO(g) ? Ni(s) + CO2(g) Kp = 700 Reaction C: CO2(g) + H2(g) ? CO(g) + H2O(g) Kp = ? Calculate the Kp value for Reaction C at this temperature. 4) The formation of a complex ion occurs in several steps. Given the series of steps and equilibrium constants below, calculate the equilibrium constant for: A3+(aq) + 2NH2-(aq) ? A(NH2)2+(aq) A3+(aq) + NH2-(aq) ? ANH2^2+(aq) K1 = 200 ANH2^2+(aq) + NH2-(aq) ? A(NH2)2+(aq) K2 = 125

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Chemistry: Structure and Properties
Nivaldo Tro 2nd Edition
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2) A + B ⇌ AB K1 = [AB] / ([A][B]) = 4.0 AB + D ⇌ E + A K2 = ([E][A]) / ([AB][D]) = 3.0 B + D ⇌ E K3 = [E] / ([B][D]) = 12 Given the equations above, how were equations 1 & 2 manipulated to create equation 3? 3) Consider reactions A and B at a particular temperature: Reaction A: NiO(s) + H2(g) ⇌ Ni(s) + H2O(g) Kp = 50 Reaction B: NiO(s) + CO(g) ⇌ Ni(s) + CO2(g) Kp = 700 Reaction C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) Kp = ? Calculate the Kp value for Reaction C at this temperature. 4) The formation of a complex ion occurs in several steps. Given the series of steps and equilibrium constants below, calculate the equilibrium constant for: A3+(aq) + 2NH2-(aq) ⇌ A(NH2)2+(aq) A3+(aq) + NH2-(aq) ⇌ ANH2^2+(aq) K1 = 200 ANH2^2+(aq) + NH2-(aq) ⇌ A(NH2)2+(aq) K2 = 125
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Transcript

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00:01 Hello everyone in this question we have given three reactions the first reaction is a combines with b forming a b the equilibrium constant of this reaction is given us k1 which is given us the concentration of ab divided by concentration of a multiplied by the concentration of b the value is given as four and the next reaction is given as ab which it combines with d forming e plus a and in this case the equilibrium concession k2 is given as concentration of e multiplied by the concentration of a divided by the concentration of a b multiplied by the concentration of d and this value is given as three and the necessary reaction is given as b combines with d forming e and the equilibrium constant k3 is given are concentration of e divided by the concentration of b multiplied by the concentration of d and the value is given as turn we had to find out the relation between k1 k2 and k3 so we can write the value of k3 that is k3 will be equal to concentration of e divided by concentration of b multiplied by the concentration of d we can multiply this with a in numerator and denominator so we can write this half that is k3 will be equal to concentration of e multiplied by the concentration of a divided by concentration of b multiplied by the concentration of t multiplied by the concentration of a.
01:50 This is after multiply that is multiply with concentration of a in numerator and denominator and denominator.
02:08 Denominator.
02:09 So again we can multiply this with concentration of a b in numerator and denominator.
02:15 So this will be written as the concentration of a b divided by the concentration of a multiplied by the concentration of b again multiplied by the concentration of e the concentration of a divided by the concentration of a b multiplied by the concentration of d so this is after multiplying multiply concentration of a b in numerator and denominator and denominator denominator...
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