NEED EXPLANATIONS ON WHY THE HIGHLIGHTED ANSWERS ARE CORRECT Consider the equili
ID: 522232 • Letter: N
Question
NEED EXPLANATIONS ON WHY THE HIGHLIGHTED ANSWERS ARE CORRECT
Consider the equilibrium, 2 NOCl(g) Cl_2(g) + 2 NO(g). When 2.000 atm NOCl is placed in a tank at 500.0 K and allowed to come to equilibrium, the equilibrium partial pressure of Cl_2 is 0.226 atm. Calculate K_p. a. 0.0660 b. 0.0115 c. 0.0193 d. 52.0 e. 15.2 When solid ammonium nitrate (NH_4NO_3) dissolves in water, the temperature of the water can drop dramatically. Taking NH_4NO_3 as the system, predict the signs of the entropy change of the system (Delta S_sys) and surroundings (Delta S_surr). a. Delta S_sys is less than 0 and Delta S_surr is less than 0. b. Delta S_sys equals 0 and Delta S_surr is less than 0. c. Delta S_sys is greater than 0 and Delta S_surr is less than 0. d. Delta S_sys is less than 0 and Delta S_surr is greater than 0. e. Delta S_sys is greater than 0 and Delta S_surr is greater than 0.Explanation / Answer
1)
2NOCl(g) <—> Cl2(g) + 2NO (g)
2.000 0 0 (initial)
2.000-2x x 2x (at equilibrium)
Given at equilibrium,
p(Cl2) = 0.226 atm
so,
x = 0.226 atm
Kp = p(Cl2) * (p(NO))^2 / (p(NOCl))^2
Kp = 0.226 * (2x)^2 / (2.000 - 2x)^2
Kp = 0.226 * (2*0.226)^2 / (2.000 - 2*0.226)^2
Kp = 0.226 * 0.2043 / 2.396
Kp = 0.0193
Answer: c
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