6ISWCC Fall 2017 24. The equilibrium constant for the reaction H2(g) + I (g)--2H
ID: 546523 • Letter: 6
Question
6ISWCC Fall 2017 24. The equilibrium constant for the reaction H2(g) + I (g)--2HI(g) is 62.5 at 800 K what is the equilibrium concentration of l2 if at equilibrium (HI] 0.21 M and (H] 0.13 M 4) a.5.4x103 M b.0.29M c.5.2x10'M d.0.21M .2.6x10 M 25. Carbon monoxide is toxic because it can successfully compete with oxygen for hemoglobin (Hb) sites according to the following equilibrium Hb(02)4(aq) + 4C0(g)--Hb(CO)4(aq) + 402(g) From Le Châtelier's principle, CO poisoning is reversed by (2) (a) increasing the O2 pressure. (b) decreasing the amount of Hb. (c) increasing the CO2 pressure. (d) increasing the CO pressure. (e) increasing the amount of Hb. 26. What effect will spraying liquid water into the equilibrium given below have if NH, is far more soluble in water than is N2 or H2? (2) N2(g) + 3H2(g) 2NH3(g) (a) More NHs(g) will form. (b) More H>(g) will form. (c) Less NHs(g) will form. (d) This will not affect the system. (e) More N2(g) will form. 27. In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products? (2) (a) 2H-8)+ O(8) 2H,0(g) (b) NO.g+CO(g)NOE)+ CO08) (c) H2(g) +12(g)2HI(g) (d) 200g)-302(g) (e) MgCO3(s)-MgO(s) + COtg)Explanation / Answer
24. H2(g) + I2(g) <====> 2HI(g)
Kc = [HI]^2/[H2][I2]
62.5 = 0.21^2/(0.13*X)
X = [I2] = 5.43*10^-3 M
answer: a
25. from lechateliers principle: any system at equilibrium undergoes stress,the equilibrium shifts,in such a direction in order to undo the stress.
answer: a
increasing the O2 pressure , makes the equilibrium shift to left,so that Hb(o2)4 Concentration increases.
26. as NH3 is soluble in water,partial pressure of NH3(g) decreases,so that equilibrium shifts to right,formation NH3 takes place.
answer: a
27. by decreasing the volume of container,partial pressure of gases increases.so that equilibrium shift towards less no of moles(if Dn is not euals to zero)
answer: a
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