The equilibrium 2no(g)+cl2(g)⇌2nocl(g) is established at 500 k. an equilibrium mixture of the three gases has partial pressures of 9.10×10−2 atm , 0.174 atm , and 0.24 atm for no, cl2, and nocl, respectively. part apart complete calculate kp for this reaction at 500.0 k. express your answer using two significant figures. kp = 40 previous answers correct part b if the vessel has a volume of 6.00 l , calculate kc at this temperature. express your answer using two significant figures.

For A: The for the given reaction is

For B: The for the given reaction is 1642.

Explanation:

The given chemical reaction follows:

The expression of for the above reaction follows:

We are given:

Putting values in above equation, we get:

Hence, the for the given reaction is

Relation of with is given by the formula:

where,

= equilibrium constant in terms of partial pressure =

= equilibrium constant in terms of concentration = ?

R = Gas constant =

T = temperature = 500 K

= change in number of moles of gas particles =

Putting values in above equation, we get:

Hence, the for the given reaction is 1642.

- "the choice that is not an indicator of a chemical change is "state of matter changes". more common than not, chemical reactions produce energy in the form of light or heat. along with energy, they also produce a new substance called the product that could be in any state of matter (solid, gas, or liquid)."

thats how its supposed to be