Express the equilibrium constant for the following Pb (NO_3)_2 Nal(aq) pbl_2 (s)

Question

Express the equilibrium constant for the following Pb (NO_3)_2 Nal(aq) pbl_2 (s) * 2 NaNO_3 (aq) K = [2NaNO_3]^2/[pb(NO_3)_2][2Nal]^2 K = [2 NaNO_3]^2[2 Nal]^2/[pb(NO_3)_2][2Nal]^2 K = [NaNO_3]^2[2 Nal]^2/[pb(NO_3)_2][Nal]^2 K = [pb (NO_3)_2][Nal]^2/[NaNO_3]^2 K = [NaNO_3]^2/[pb(NO_3)_2][Nal]^2 Determine the value of K_c for the following reaction if the equilibrium concentration are as follows HCl(g) + I_2(s) 2 HI(g) Cl_2(g) 2.8 * 10^31 3.5 * 10^-32 1.2 * 10^17 8.2 * 10^-18 1.4 * 10^-19 Consider the following reaction at equilibrium. what will happen if O_2 is added to the reaction? 4 FeS_2(s) * H O_2(g) 2 Fe_2O_3(s) * 8 SO_2(g) The equilibrium constant will increase. The equilibrium will change in the direction of the reactants. The equilibrium will change in the direction of the products. No change in equilibrium is observed. The equilibrium constant will decrease. Consider the following reactions: Xe(g) * 2 F_2 (g) XeF_4 (g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F_2. If the equilibrium pressure of is 0.34 atm, find the equilibrium constant (k_p) for the reaction. 0.99 0.12 0.040 8.3 23

Explanation / Answer

Question 15.

Note that we must always include aqueous solutions, and ignore liquids + solids, since those have activities of 1

then

K = [products]^p /[reactants]^r

K = [PbI2][NaNO3]^2 /([Pb(NO3)2][NaI]^2)

[PBI2] = 1

K = [NaNO3]^2 /([Pb(NO3)2][NaI]^2)

best answer is E

Q16

Kc for:

K = [HI]^2]Cl2]/([HCl]^2[I2])

K = [HI]^2[Cl2]/([HCl]^2)

K = (5.6*10^-16)^2(0.0019)/(0.13^2)

K = 3.52*10^-32

nearest answer is B

Q17

If we add O2 to the system, the reactants increases in concentration

Meaning that the equilibrium must shift toward the right, so more products will be produced

Note that the equilibrium constant is always constant, so only equilbrium shifts to products is seen

choose C

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