K,-.M 2SOMg) +0(g) s 2 soug) Consider the equilibrium. Calculate the 1. value of
ID: 694829 • Letter: K
Question
K,-.M 2SOMg) +0(g) s 2 soug) Consider the equilibrium. Calculate the 1. value ofQ" for a situation siruation in which the concentrations are [sO] -2.00 M. toJ-1.50 M, and t So-1.25M Does this mixture shift toward the reactants or products to reach equilibrium? Study the discussion in your textbook about comverting K, and K, Write the K, expression for the reaction in question I and calculate its value at "C. Remember, R-0.0821 L atm/mol- K 2. 3. Consider the equilibrium PCl(g)+ Cl(g)PCL,(g). How would the following changes affect the partial pressures of each gas at equi librium? PCL(g)+Cl(g)PClg) a) addition of PCl b) removal of Cl c) removal of PCl, d) decrease in the volume of the container addition of He without change in volume e) How will each ofthe changes in question 3 affect the Keo (1-increase, -decrease; 4, --unchanged) 5. Indicate how each of the following changes affects the amount of each gas in the system below, for which Heation 9.9 kcal. H(g) +CO-(g) H0(g)+CO(g) a) addition of CO b) addition of HO c) addition of a catalyst increase in temperature decrease in the volume of the container d) e) 6. How will each of the changes in question 5 affect the equilibrium constant?Explanation / Answer
Q1
Q = [products]^p / [reactants]^r
Q = (SO3)^2 / (SO2)^2*O2
Q = ( 1.25^2)/((2^2)(1.5))
Q = 0.260416
since Q < K, then this must go towards left side, tht is, there is enough SO3 to go reverse reaciton and produce SO2 and O2
Q2
Kp for:
Kp = Kc*(RT)^dn
dn = 2 - (1+2) = 2-3 = -1
Kp = (4.36)(0.082*283)^-1
Kp = 0.1878
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