Consider the equilibrium 4NH; (g) + 502 (g) ANO (8) + 611, 0(8) Which one of the followings will shift the equilibrium to the left? (a) Adding NHs. (b) Pressure is decreased by increasing the volume. (c) Temperature is decreased. (d) A catalyst is added. (e) None of the above. =

Consider the equilibrium 4NH; (g) + 502 (g) ANO (8) + 611, 0(8) Which one of the followings will shift the equilibrium to the left? (a) Adding NHs. (b) Pressure is decreased by increasing the volume. (c) Temperature is decreased. (d) A catalyst is added. (e) None of the above. =

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat....

See similar textbooks

Similar questions

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 2NO(g)N2(g)+O2(g)K=11031 For each reaction, assume some quantities of the reactants were placed in separate containers and allowed to come to equilibrium. Describe the relative amounts of reactants and products that would be present at equilibrium. At equilibrium, which is faster, the forward or reverse reaction in each case?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)