Chemistry, 07.04.2021 08:10 roadrnr8970

The equilibrium 2NO(g)+Cl2(g)⇌2NOCl(g)
is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 9.20×10−2 atm , 0.176 atm , and 0.29 atm for NO, Cl2, and NOCl, respectively.

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Kp = 41.53Kp = 41.53Kc = 1.01Kp = 41.53Kc = 1.01Explanation:Kp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = [NOCl]^2/[NO]^2[Cl]Kp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = [NOCl]^2/[NO]^2[Cl]Kp= [0.25]^2/[0.174][0.093]^2 = 41.53Kp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = [NOCl]^2/[NO]^2[Cl]Kp= [0.25]^2/[0.174][0.093]^2 = 41.53 Kp = Kc (RT)^DnKp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = [NOCl]^2/[NO]^2[Cl]Kp= [0.25]^2/[0.174][0.093]^2 = 41.53 Kp = Kc (RT)^DnHence, Kc = Kp/[RT]^(delta n )^-1Kp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = [NOCl]^2/[NO]^2[Cl]Kp= [0.25]^2/[0.174][0.093]^2 = 41.53 Kp = Kc (RT)^DnHence, Kc = Kp/[RT]^(delta n )^-1n = sum of the number of moles of products minus the sum of the number of moles of reactants= 2-3 = -1 in this caseKp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = [NOCl]^2/[NO]^2[Cl]Kp= [0.25]^2/[0.174][0.093]^2 = 41.53 Kp = Kc (RT)^DnHence, Kc = Kp/[RT]^(delta n )^-1n = sum of the number of moles of products minus the sum of the number of moles of reactants= 2-3 = -1 in this caseKc = 41.53/(0.0821 * 500)^1Kp = 41.53Kc = 1.01Explanation:To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:Kp = [NOCl]^2/[NO]^2[Cl]Kp= [0.25]^2/[0.174][0.093]^2 = 41.53 Kp = Kc (RT)^DnHence, Kc = Kp/[RT]^(delta n )^-1n = sum of the number of moles of products minus the sum of the number of moles of reactants= 2-3 = -1 in this caseKc = 41.53/(0.0821 * 500)^1Kc = 1.01

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The equilibrium 2NO(g)+Cl2(g)⇌2NOCl(g)
is established at 500 K. An equilibrium mixture of th...

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