Consider the following generic reaction: A + 2 B ? C + D If...

Consider the following generic reaction: A + 2 B ? C + D If this reaction is carried out using 3.0 moles of A and 5.0 moles of B, a. What is the limiting reagent in the reaction? b. How many moles of C are formed in this reaction?

Transcript

00:01 At equilibrium, the forward and backward rates of the reaction are equal.

00:05 As a consequence, the concentration or the amount of the substances in the reaction no longer changed.

00:11 We can then establish the ratio of the amount of the product to that of the reactor using an equilibrium constant.

00:17 In this problem, we're given with the demerization reaction of nitrogen dioxide to form dinitrogen tetroxide according to this.

00:30 Balanced chemical equilibrium equation now if we start with 14 .8 moles so it should be your initial moles of n02 and it is found that at equilibrium the most left for this or the most that are of the product formed is five moles so of course initially there's none of the product so what do you want to establish are the following so for letter a well there's just one actually we're going to find the kc and as well as the kp so these are two equilibrium constants just expression different quantities so k c is for when you're expressing it in terms of concentrations and kp is when you're expressing it in partial pressures if the reaction happens at 400 kelvin and in a reaction vessel which volume is equal to three three liters so let us first establish the or complete the initial change and equilibrium table so in other words this is the ice so if we assume that there are 2x most of n02 that are the react then we have x moles of n204 that is formed so that's based on the balanced chemical equation so the equilibrium will be 14 .8 minus 2x since the amount the reactor must increase and the equilibrium amount of the product will be equal to x since that's going to be initial plus the change and that x is equal to 5 as we established here therefore if x is equal to 5 it follows therefore that the most of n o2 that equilibrium which we have as 14 .8 minus 2 x will be equal to 14 .8 minus 2 x will be equal to 14 .8 minus 2 times 5 for this way to be 4 .8 so this is the most of n02 at equilibrium and most of n204 again at equilibrium is given to be equal to 5 now we let's express these in terms of concentration we simply divide the most by the volume of the solution in the volume of the container in liters so for n02 we have 4 .8 divided by 3 and that and this gives us 1 .60 molar for n204 we have 5 divided by 3 and that gives us 1 .67 now ac which is the equilibrium concept in terms of concentrations of in terms of polarity is solved as the ratio of the equilibrium constitution of the product raised to its respective coefficient in the balance equation to that of the constitution at equilibrium of the reactant raised to its coefficient in the balance equation so we're going to raise no2 to 2 because that's the coefficient of no2 in the balance equation so therefore you have 1 .67 divided by 1 .60 squared giving us kc that is equal to 0 .0 651 so this is your casey now kp can be expressed in terms of kc as follows so kp is equal to kc times r t raised to the bar delta n where r is the gas constant that's going to be 0 .08 to 1 liter atm for more kelvin your temperature is the your t is the temperature in kelvin and your delta n is the difference in the most of the product gaseous product to the most of the gaseous reactants.

04:49 So we'll take the, we will base that on the coefficient of the gaseous species in the balance equation...

Question

Consider the following generic reaction: A + 2 B ? C + D If this reaction is carried out using 3.0 moles of A and 5.0 moles of B, a. What is the limiting reagent in the reaction? b. How many moles of C are formed in this reaction?

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