The two equilibrium constants for the same reaction, K_ and K_p, will always equ
ID: 538313 • Letter: T
Question
The two equilibrium constants for the same reaction, K_ and K_p, will always equal one another when A. all of the reactants and products are gases. B. in the reaction equation, the number of moles of gaseous products is smaller than the number of moles of gaseous reactants. C. in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants. D. in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants. E. in the reaction equation, the total number of moles of reactants equals that of the products. What is the mass-action expression, Q_ for the following reaction? Sb F_5(g) + 4 Cl_2 (g) doubleheadarrow SbCl_3 (g) + 5 ClF (g) A. (P_, X_)^5/(P_Cl_)^4 (P_) B. (P_)^4 (P_)/(P_ XP_)^5 C. (P_, XP_)/(P_, XP_) D. (P_, XP_)/(P_, XP_) E. None of these is Q_v Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached, P_NO = 0.526 atm, P_Br2 = 1.59, and P_OBr = 7.68 atm. Calculate K_p for the reaction: 2 NO(g) + Br_2 (g) doubleheadarrow 2NOBr(g) A. 91.8 B) 134 C) 7.45 times 10^-5 D) 0.109 E) 9.18 CS_2 (g) + 3 Cl_2 (g) doubleheadarrow CCl_4 (g) + S_2 Cl_2 (g) At a given temperature, this reaction is at equilibrium where [CS_2] = 0.050 M, [Cl_2] = 0.25 M, [CCl_4] = 0.15 M, and [S_2 Cl_2] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS_2 = 0.15 M, Cl_2 = 0.18 M, CCl_4 = 0.29 M, and S_2 Cl_2 = 0.21 M? A) no change B) cannot predict unless we know the temperature C) to the left D) to the right E) cannot predict unless we know whether the reaction is endothermic or exothermic Nitrogen gas (N_2) reacts with hydrogen gas (H_2) to form ammonia (NH_3). At 200 degree C in a closed 1.0 atm of nitrogen gas is mixed with 2.0 atm of hydrogen gas. At equilibrium, the total pressure is 2.2 a Calculate the partial pressure of hydrogen gas at equilibrium. A) 0.0 atm B) 2.2 atm C) 0.80 atm D) 1.4 atm E) none of these Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO_2 (g) doubleheadarrow 2 NO (g) + O_2 (g): delta H degree_ = Under which reaction conditions would you expect to produce the largest amount of oxygen? A. high temperature, high pressure B. low temperature, high pressure C. low temperature, low D. high temperature, low pressure E. none of these, unless a catalyst is presentExplanation / Answer
Question 8.
Kc and Kp can be related as follows:
Kp = Kc*(RT)^dn
where dn is the change of moles of GASES, so
dn = moles of gas in products - moles of gas in reactants
therefore, the only way
Kp = Kc, is when dn = 0, so RT^0 = 1, and Kp = Kc*1
so
choose "D"
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