How do you figure out the answer for the reverse reaction? At 350 K the value of Kp for the equilibrium represented by the balanced equation is 2.87 x 10-2. Calculate the value of Kc for the reverse reaction at the same temperature. Express answer in scientific notation.

2NOBr(g) = 2NO(g)+Br2(g)

Kreverse for the reverse reaction is just 1/Kforward

That is 1/2.87 x 10^-2

To find the value of Kc for the reverse reaction at the same temperature, you need to use the relationship between Kp and Kc.

Kp represents the equilibrium constant expressed in terms of partial pressures, while Kc represents the equilibrium constant expressed in terms of molar concentrations.

The equation to relate Kp and Kc is as follows:
Kp = Kc(RT)^(∆n)

Where:
- Kp is the equilibrium constant in terms of partial pressures
- Kc is the equilibrium constant in terms of molar concentrations
- R is the ideal gas constant (usually 0.0821 L·atm/mol·K)
- T is the temperature in Kelvin
- ∆n is the difference in the number of moles of gaseous products and reactants (moles of products - moles of reactants)

In this case, the balanced equation for the given reaction is:
2NOBr(g) = 2NO(g) + Br2(g)

From the equation, you can see that ∆n is equal to 3 - 2 = 1, as there is a total of 3 moles of gaseous products and 2 moles of gaseous reactants.

Given that Kp = 2.87 x 10^(-2) and the temperature is 350 K, we can calculate Kc using the equation mentioned earlier.

1. Convert Kp to Kc:
Kp = Kc(RT)^(∆n)
Kc = Kp / (RT)^(∆n)

2. Plug in the values:
Kc = (2.87 x 10^(-2)) / [(0.0821 L·atm/mol·K) * (350 K)]^(1)

3. Calculate the value:
Kc = (2.87 x 10^(-2)) / (28.5275)
Kc = 1.004 x 10^(-3)

Therefore, the value of Kc for the reverse reaction at the same temperature is 1.004 x 10^(-3) (expressed in scientific notation).