Consider first photo but answer only 3 and 4 ASAP Please!! O ProcurarEquilibrium v 2021 KS..-quemaReferênciasCorreioReverVerAjudaA A Aa A E-E-E三三A TAaBbCeDdl aBbCcD AaRbCcbdFe AABE- 12AaBbCcDdEÊnfaseForteT Legenda1 NormalSubtib x, x' A- eA-EstilosParágrafoTipo de LetraThis set of questions addresses what would happen if a system at equilibrium is disturbed in different ways.Consider the reaction:N2(g) + 3 H2(g) → 2 NH3 (g)[NH,When the reaction is at equilibrium, the ratio of concentrations,is CONSTANT and this constantis called Kc. For this entire set of questions, take the value of Kc for this reaction to be 16.[NHWhen the reaction is NOT at equilibrium, the ratio[N,][H,Jcan take on just about any value.For example, if we start with all reactants and zero products, then the ratio would equal zero. When not atequilibrium, we call this ratio Qc. It is referred to as the "reaction quotient".So, in summary:Qc can be any valuewhen the reaction is notWhen the reaction is at equilibrium K, -[NH;]- = 16.at equilibrium.The value of Qc justdepends on the[NH,][N J[H,When the reaction is NOT at equilibrium, Qc =#Constantconcentrations of the R'sand P's in the reaction(1) If the concentrations of the reactants and products are as follows:[N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00 M .. is this system at equilibrium?Prove your answer by figuring out the value of Qc and seeing if it equals 16. If itdoes, the reaction is at equilibrium.mixture.(2) Suppose you increase the concentration of N2 from 1.00M to 2.00 M, leaving[H2] =1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way will the reaction go?First: What would LeChatelier's Principle say?To prove your answer, calculate the new reaction quotient, Qc.Is Qcgreater than, less than, or equal to Kc? (Circle one).If Qc is not equal to Kc, what would have to happen to make it equal 16?stados Unidos)Concentração ESLITOSParágrafoTipo de Letra(3) Suppose that instead of adding N2, as in (2), you increase the concentration of H2 from 1.00 M (in #1) to2.00 M, leaving [N2] = 1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way willthe reaction go? First: What would LeChatelier's Principle say?To prove your answer, calculate the new reaction quotient, Qc.Is Qcgreater than, less than, or equal to Kc? (Circle one).If Qc is not equal to Kc, what would have to happen to make it equal 16?(4) Can you make a general statement about what happens to a reaction at equilibrium when you add eitherreactant? How would this be different for a reaction that "goes to completion"?13(5) In the lab, we added a great excess of one reactant and stated that this would make the reaction goalmost all the way to the right (to completion). This question uses the above reaction to explore thisphenomenon. Suppose you start with the reactants at equilibrium with concentrations as in (#1):[N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00MDConcentraçãoidos)

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Consider first photo but answer only 3 and 4 ASAP Please!! O ProcurarEquilibrium v 2021 KS..-quemaReferênciasCorreioReverVerAjudaA A Aa A E-E-E三三A TAaBbCeDdl aBbCcD AaRbCcbdFe AABE- 12AaBbCcDdEÊnfaseForteT Legenda1 NormalSubtib x, x' A- eA-EstilosParágrafoTipo de LetraThis set of questions addresses what would happen if a system at equilibrium is disturbed in different ways.Consider the reaction:N2(g) + 3 H2(g) → 2 NH3 (g)[NH,When the reaction is at equilibrium, the ratio of concentrations,is CONSTANT and this constantis called Kc. For this entire set of questions, take the value of Kc for this reaction to be 16.[NHWhen the reaction is NOT at equilibrium, the ratio[N,][H,Jcan take on just about any value.For example, if we start with all reactants and zero products, then the ratio would equal zero. When not atequilibrium, we call this ratio Qc. It is referred to as the &#34;reaction quotient&#34;.So, in summary:Qc can be any valuewhen the reaction is notWhen the reaction is at equilibrium K, -[NH;]- = 16.at equilibrium.The value of Qc justdepends on the[NH,][N J[H,When the reaction is NOT at equilibrium, Qc =#Constantconcentrations of the R'sand P's in the reaction(1) If the concentrations of the reactants and products are as follows:[N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00 M .. is this system at equilibrium?Prove your answer by figuring out the value of Qc and seeing if it equals 16. If itdoes, the reaction is at equilibrium.mixture.(2) Suppose you increase the concentration of N2 from 1.00M to 2.00 M, leaving[H2] =1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way will the reaction go?First: What would LeChatelier's Principle say?To prove your answer, calculate the new reaction quotient, Qc.Is Qcgreater than, less than, or equal to Kc? (Circle one).If Qc is not equal to Kc, what would have to happen to make it equal 16?stados Unidos)Concentração ESLITOSParágrafoTipo de Letra(3) Suppose that instead of adding N2, as in (2), you increase the concentration of H2 from 1.00 M (in #1) to2.00 M, leaving [N2] = 1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way willthe reaction go? First: What would LeChatelier's Principle say?To prove your answer, calculate the new reaction quotient, Qc.Is Qcgreater than, less than, or equal to Kc? (Circle one).If Qc is not equal to Kc, what would have to happen to make it equal 16?(4) Can you make a general statement about what happens to a reaction at equilibrium when you add eitherreactant? How would this be different for a reaction that &#34;goes to completion&#34;?13(5) In the lab, we added a great excess of one reactant and stated that this would make the reaction goalmost all the way to the right (to completion). This question uses the above reaction to explore thisphenomenon. Suppose you start with the reactants at equilibrium with concentrations as in (#1):[N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00MDConcentraçãoidos)

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