Methyl alcohol can be prepared commercially by the reaction of hydrogen with carbon monoxide. Under equilibrium conditions at 7.00 × 102 K,

[H2] = 0.0720 M, [CO] = 0.200 M, and [methanol] = 0.0300 M. Find the value of Kc, and then find the value of Kp. What is the value of Kp?
1. 1.05 × 10-6 4. 4.39 × 10-2
2. 7.33 × 10-6 5. 8.76 × 10-3
3. 1.14 × 10-1 6. none of the above

I found the value of Kc to be 28.9. I know to convert Kc to Kp, the equation is Kp=KC(RT)deltaN
I thought that deltaN may be the stoichiometric coefficients from the equation Co+2H2-->CH3COH, like products-reactants and when I do that I get -2. If I plug all those values in I get 28.9(8.314*700)^-2, which is 8.53*10^-7. Am I doing something wrong? I know it could be none of the above, i'm nervous that it isn't close to any answers.

To find the value of Kp, you are correct in using the equation Kp = Kc(RT)^(Δn), where Kc is the equilibrium constant in terms of concentrations, R is the gas constant, T is the temperature in Kelvin, and Δn is the change in the number of moles of gas from reactants to products.

In this case, the reaction is CO + 2H2 -> CH3OH. From the balanced equation, you can see that there are 2 moles of gas on the reactant side (CO and 2H2) and 1 mole of gas on the product side (CH3OH). So Δn = 1 - 2 = -1.

Now, let's calculate Δn. The gas constant, R, is 0.0821 L·atm/mol·K, and the temperature, T, is 700 K.

Kp = Kc(RT)^(Δn)
Kp = 28.9 (0.0821 L·atm/mol·K)(700 K)^(-1)
Kp ≈ 28.9 (0.0821/700)
Kp ≈ 0.341

Therefore, the value of Kp is approximately 0.341. None of the answer choices provided match this value, so none of the above is the correct answer.

It's important to note that the actual answer may be rounded differently in the given options, so it's always possible that an answer choice may not be an exact match. However, based on your calculations, none of the provided choices seem to match the calculated value closely.