Nitric oxide reacts with chlorine gas according to the following reaction:
2NO(g)+Cl2(g)?2NOCl(g)
Kp=0.27 at 700 K
A reaction mixture initially contains equal partial pressures of NO and Cl2. At equilibrium, the partial pressure of NOCl was measured to be 110 torr. What were the initial partial pressures of NO and Cl2?

The initial partial pressures of and are 134 torr each.

Explanation:

The given balanced equilibrium reaction is,

Initial pressure             x          x                 0

At eqm. conc.        (x-2y)       (x-y)             2y

The expression for equilibrium constant for this reaction will be,

we are given : 2 y= 110 torr

y = 55 torr

Now put all the given values in this expression, we get :

Thus the initial partial pressures of and are 134 torr each

b.false that your answer

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally