MasteringChemisty Chap 10 eam part2-Google Chrome Secure https://session.masteri

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MasteringChemisty Chap 10 eam part2-Google Chrome Secure https://session.masteringchemistry.com/myct/itemView?assignmentProblemID-88981819 Chap 10 exam part 2 Item 1 Time Remaining: 00:56:25 Hide Part A - 2 NH3 (g)+ 46 KJ > N2 (0) + 3H2 (0) For the reaction at equilibrium given above, give 2 ways that you can shift the equibrium to the left. Essay answers are limited to about 500 words (3800 characters maximum, including spaces) 3800 Character(s) remaining Submit My Answers Give Up Part B-2 NH3 (9) + 46 KJ N2 () +3H2 (g) For the reaction at equilbrium given above, calculate the numeric value of Kc if the concentrations at equilibrium are 0.5 Essay answers are limited to about 500 words (3800 characters maximum, including spaces). 3800 Character(s) remaining Submit My Answers Give Up Part C -Are all reversible reactions at equilibrium? Explain why or why not Essay answers are limited to about 500 words (3800 characters maximum, including spaces). 3800 Character(s) remaining

Explanation / Answer

Question-1

Equilibrium of Haber process

N2 + 3H2 ----------2 NH3+ 46 kJ

To shift the equilibrium towards right side, Or to produce maximum amount of ammonia , which factors can be changed?

1. Increase the concentration of reactants (Nitrogen and hydrogen), then the reaction will shift towards right side(product side) by increasing the rate of forward reaction. That is according to Le Chatelier's principle, if the concentration of reactants increased in a reversible reaction, then that system will try to cancel the change(or will try to decrease the concentration of reactant by increasing forward reaction ) on concentration.

2. Pressure:-

4 moles of reactant (1 N2 and 3 H2) will give 2 moles of products. If the pressure of the system increases, then system will try to decrease the pressure by favoring the reaction in which number of moles of particles are lowering. That is, forward reaction will take place and the number of moles of reactant reduce from 4 to 2. So increases the pressure of the system to get maximum amount of ammonia or NH3.

question-2

Kc or equilibrium constant = [NH3]2 / [N2][H2]3

given that, concentration at equilibrium = 0.5 for all

then Kc = [0.5]2 / [0.5][0.5]3 =[0.5]-2 =4

Question-3

A reaction become reversible only if both forward(reactant- products) reaction and backward reaction(product--reactant) take place in a reaction system. An equilibrium is a stage at which both the rate of forward reaction and backward reaction are equal. So every reversible reaction should have such an equilibrium point, but will not always. If the factors affecting the equilibrium of a reaction, like concentration, temperature, pressure are unique for both reactants and product, then that system will be in equilibrium.

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