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Posted: Tue Nov 28, 2017 9:14 pm
For the reaction N2(g) + 3H2(g) <-> 2NH3(g) at 400K, K= 41. Find the value of K for each of the following reactions at the same temperature.
a) SO2(g) + 1/2O2(g) <-> SO3(g)
b) SO3 <-> SO2(g) +1/2O2(g)
c) 3SO2(g) + 3/2O2 <-> 3SO3(g)
(Claire Woolson Dis 3J)
Posted: Wed Nov 29, 2017 12:34 am
You wrote the question wrong. I think you combined portions of 11.37 and 11.38.
Posted: Wed Nov 29, 2017 10:22 am
To find the change to the value of K, you have to write the formula for the concentration. It doesn't necessarily matter what the concentrations of the products and reactants are, because we know the final value of K. To calculate this change, you use the coefficients. So if the chemical equation is multiplied through by 2, you know that when you write out the formula for K the exponents on the concentrations of products and reactants will also double. This means that you are going to square the value of K. Similarly, if the chemical equation is multiplied through by 1/2, the exponents will also decrease by 1/2. This means that you are going to take the square root of K. It's all about the relationship between the coefficients and the concentration formula!