Log in. And we want to determine what the value is of KP at the same temperature. Times are t to the power of delta and gas. So when we go to solve for KP, we plug in that given value of K C, which is 2. Our is the ideal gas constant which is 0. Leaders times atmospheres, her mole times Kelvin T is thedc richer, which, when we convert into killed in, comes out to and now we raise our T to the power of delta and gas.
We consult the reaction to determine delta and gas. We see we have to total moles of gas on the product side in two plus one. So three total moles of gas on the react inside, so two minus three comes out to negative one for delta and gas. So you raise our times t to the power of negative one. And when we plug that all in, we should get a final answer for the value of K P at this temperature for this reaction to be about 1.
View Full Video Already have an account? Determine the values of K p that correspond to the following values of K c. Reversing the reaction gives the proper reactants and products for the target reaction, but with the wrong stoichiometry.
Reversing the reaction also means that the new equilibrium constant is the inverse of the original equilibrium constant. This means that the new equilibrium constant is the square root of the old equilibrium constant. First, find K p for the target reaction using the Law of Multiple Equilibria.
The target reaction has 2 CH 4 g as one of the reactants and 1 C 2 H 2 g as a product. This tells us that the first reaction must have all of the stoichiometric coefficients doubled and that the K p for the given reaction must be squared.
The stoichiometric coefficients of the second reaction must all be halved and then the reaction reversed so this changes the K p to the inverse of the square root of the given reaction. The sum of these two reactions is given below, which conveniently eliminates CO g. K p for the summed reaction is found by multiplying the two equilibrium constants. This is not the target reaction. To reach the target, the third reaction given above must be used with all of its stoichiometric coefficents multiplied by three.
This means that the equilbrium constant must be cubed. Now, adding the last two reactions together gives the target reaction. K p for the target reaction is found by multiplying equilibrium constants.
Since the equilibrium constant data is given in terms of K p for the known reactions, first find K p for the unknown reaction and then, lastly, convert it to K c. Reaction 1 has nitrogen and oxygen as reactants but a wrong product. Reaction 3 can be used to eliminate the nitrogen dioxide product from 1 and also introduces chlorine:.
The NO 2 g found on both reactants and products sides has been eliminated. This has all the correct reactants, but the product is wrong and the stoichiometry is not quite right.
Adding 4 and 2 rev gives the desired reaction, both eliminating the NO 2 Cl and correcting the stoichiometry. The equilibrium concentrations of each component is given, so can be directly put into the mass action expression to give.
In a sealed 1. Problem 5. Problem 6. Problem 7. Problem 8. Problem 9. Problem Video Transcript were given this reaction as well as the value for the equilibrium constant K c at a certain temperature.
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