Consider the following equilibrium.2 nobr(g)< => 2 no(g) + br2(g)if nitrosyl bromide, nobr, is 34 percent dissociated at 25°c and the total pressure is 0.25 atm, calculate kp and kc for the dissociation at this temperature.

of the reaction is  .

of the reaction is  .

Explanation:

Initial pressure of NOBr is "x" atm.

34% = 0.34

The equilibrium chemical reaction is a follows.

Initial          x                                      0          0

Change    -0.34x                             +0.34x    +0.17x

Final        (x-0.34x)                          +0.34x     +0.17x

Total pressure = sum of the pressure at equilibrium.

Partial pressure of NOBr=  x-0.34x =x (1-0.34)

= 0.213(0.66) = 0.14 atm.

Hence, partial pressure of is 0.14 atm.

From equation (1)

Therefore, of the reaction is  .

Rearrange the equation is as follows.

= number of moles of reactants - Number of moles of products

= 3-2 = 1

Therefore, of the reaction is  .

is it a purebred? it looks more like a red nose, but it doesn't have the red could it be a staffordshire bull terrior? unsure if that's the right name for it sorry