chlorinpoints) The equilbrium constant for the formation of nitrosylchloride fro

Question

chlorinpoints) The equilbrium constant for the formation of nitrosylchloride from nitric oxide and 2NO(g) Cla (g) 2NOCI(g) is 6.5 x 10 at 35 c and whether the reaction will proceed to the right or to the left to achieve equilibrium when the starting pressures are PNO atm, 0.42 and PNoor 1.76 atm. 2. (15 Points) For each of the following equilibria, write the equilibrium constant for Ko Where appropriate, also write the equilibrium constant for Ko a. 2NaHsos(s) at Nason (s) H2O(g) Sos(g) b. s) 2HF(g) at CaFiz (s) HaO(g) CO(g) c. AgCKs) +Br" (aq) AgBr(s) Cl (aq)

Explanation / Answer

1)

T = 35.0 oC =(35.0 + 273) K

= 308.0 K

n = number of gaseous molecule in product - number of gaseous molecule in reactant

n = -1

Kp= Kc (RT)^ n

Kp = 65000.0*(0.0821*308.0)^(-1)

Kp = 2.571*10^3

Answer: Kp = 2.6*10^3

Now for given pressures,

Qp = p(NOCl)^2 / {p(NO)^2 * p(Cl2)}

Qp = 1.76^2 / (1.01^2 * 0.42)

Qp = 7.23

Since Qp<Kp —> The equilibrium will move to right to establish equilibrium

Answer: to the right

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