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Consider the following reaction at equilibrium:$$\mathrm{A}(g) \rightleftharpoons 2 \mathrm{B}(g)$$From the data shown here, calculate the equilibrium constant (both $K_{P}$ and $K_{\mathrm{c}}$ ) at each temperature. Is the reaction endothermic or exothermic?$$\begin{array}{ccc}\text { Temperature }\left(^{\circ} \mathrm{C}\right) & {[\mathrm{A}](M)} & {[\mathrm{B}](M)} \\200 & 0.0125 & 0.843 \\300 & 0.171 & 0.764 \\400 & 0.250 & 0.724\end{array}$$

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exothermic

Chemistry 102

Chapter 14

Chemical Equilibrium

Drexel University

University of Kentucky

University of Toronto

Lectures

10:03

In thermodynamics, a state of thermodynamic equilibrium is a state in which a system is in thermal equilibrium with its surroundings. A system in thermodynamic equilibrium is in thermal equilibrium, mechanical equilibrium, electrical equilibrium, and chemical equilibrium. A system is in equilibrium when it is in thermal equilibrium with its surroundings.

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In chemistry, chemical equilibrium (also known as dynamic equilibrium) is a state of chemical stability in which the concentrations of the chemical substances do not change in the course of time due to their reaction with each other in a closed system. Chemical equilibrium is an example of dynamic equilibrium, a thermodynamic concept.

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Consider the following rea…

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Consider the reaction:…

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Consider the following equ…

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for this problem. We have three temperatures for which we need to solve a for a Casey and a K p value. Because the concentrations were given to us. The first que value for which we will solve will be the Casey value. And then, from there we can get the KP value. So a 200 degrees Celsius with this being our reaction in the Casey value being equal to the product be concentration squared, divided by the product. A. We'll take the product, be concentration and square it divided by the reactant a concentration. And we get 56.9 to get the KP value from the Casey value, it'll be a K P. Value is equal to the Casey value multiplied by the are, which is the universal gas constant multiplied by the temperature would in Kelvin. So it'll be the 200 plus the 2 73 And then the whole thing is raised to the Delta End and Delta and will be the two moles of product minus the one mole of reactant, and we get 2200. We'll do the same thing at 300 degrees Celsius. Recognizing here the product concentration be is 0.764 which will square and in the reactant concentration A is 0.171 We get 3.41 Then our KP value is going to be equal to the Casey value multiplied by r T raised to the one the temperature now is 300. So it'll be 300 plus 2 73 to get art Kelvin temperature and we get 100 and 61 that at 400 degrees Celsius thes ahrar concentrations. We get a Casey value of 2.1. Then to get the KP value will do the same thing K p is equal to Casey multiplied by rt Race of Delta, in which we established with one and we get 116. So we see that as we are increasing the temperature were decreasing the KP value when we increased temperature and decrease cape, the KP value or the Casey value. This corresponds to an exo thermic reaction

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