Consider the reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) Kp = 28.4 at 298K In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 126 torr. What is the partial pressure of NOBr in this mixture?

Video transcript

Hello everyone today we are being given a problem and asked to calculate the concentration of oxygen, gas at equilibrium for the mixture. So we have different concentrations for different products and reactant and then we have our chemical equation here which is thankfully balanced for us. And then we have a K E Q value of 5 60. So the first thing we wanna do, the first thing we wanna do is write out our que e que expression. So for a k E cube expression we're only gonna include compounds that are in a gas or a an acquis form. And so in the numerator we're going to put in our brackets whatever our products are. And then denominator we're going to write our reactant. So we have S. 03 in the numerator and we have that coefficient of two. So that coefficient becomes that exponent For our denominator. We have s. 0. 2 and we have a two as the coefficient for S. 02. So we're going to write to is the exponent there And then we're going to multiply that in brackets with 02. That does not have a Coefficient. So there is no explanation for 02. Next we're simply going to plug in our values that we're given. So our cake here we know is 560. We're gonna say that equals are Concentration of S. 03 which is 9.20. We're going to square that And then the denominator. We're going to write our concentration for S. 02 which is 3.50. We're gonna square that and our concentration for 02 is what we are trying to find. Simple Algebra will yield us a concentration for oxygen as 0.012 bowler as our final answer. I hope this helps, and until next time.