Question

Based upon equations (1) and (2) below, how could one express the equilibrium constant 10 for...

Based upon equations (1) and (2) below, how could one express the equilibrium constant 10 for equation (3)?

(1) S(s) + O2(g) 6 SO2(g) equilibrium constant K1

(2) 2 SO3 6 2 SO2(g) + O2(g) equilibrium constant K2

(3) S(s) + 3/2 O2(g) 6 SO3(g) equilibrium constant K3

Homework Answers

Answer #1

The reactions

S + O2 = SO2 K1

2SO3 = 2SO2 + O2 K2

S + 3/2O2 = SO3

clearly, we need to invert reaction (2) in order to have SO3 in the right... also divide by 2, since we have a coefficient of 1

so

S + O2 = SO2 K1

2SO2 + O2= 2SO3 1/K2 (inverting makes an inverse in K as well)

S + O2 = SO2 K1

SO2 + 1/2O2= SO3 (1/K2)^(1/2) (division by 2, is equivalent to powering to the 1/2)

now..

note that if we add reaction 1 + 2 :

S + O2 + SO2 + 1/2O2 = SO2 + SO3

cancelling common terms

S + 3/2O2 = SO3

which is what we wanted

so

K3 can be expressed as

K3 = K1*(1/K2)^(1/2)

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI...
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI (b)2 NO(g) + O2(g)           2 NO2(g) (c)N2(g) + 3 H2(g)           2 NH3(g) (d) CO(g) + NO2(g)           CO2(g) + NO(g) (e) 2 CO(g) + O2(g)             2 CO2(g) 2.    Write equilibrium expressions for each of the following equilibria: (a) 2 C(s) + O2(g)                  CO(g) (b) Zn2+(aq) + H2S(g)               ZnS(s) + 2 H+(aq) (c) HCl(g) + H2O()                  H3O+(aq) + Cl–(aq) (d)H2(g) +  O2(g)                   H2O(g) 3.         Which of the following is more likely to precipitate the hydroxide ion? (a)...
Determine the value of the equilibrium constant, Kgoal, for the reaction N2(g)+H2O(g)⇌NO(g)+12N2H4(g), Kgoal=? by making use...
Determine the value of the equilibrium constant, Kgoal, for the reaction N2(g)+H2O(g)⇌NO(g)+12N2H4(g), Kgoal=? by making use of the following information: 1. N2(g)+O2(g)⇌2NO(g), K1 = 4.10×10−31 2. N2(g)+2H2(g)⇌N2H4(g), K2 = 7.40×10−26 3. 2H2O(g)⇌2H2(g)+O2(g), K3 = 1.06×10−10
Answer the following questions: (a) The equilibrium constant for the following reaction is 2.90×10-2 at 1150K....
Answer the following questions: (a) The equilibrium constant for the following reaction is 2.90×10-2 at 1150K. 2SO3(g) --> 2SO2(g) + O2(g) If an equilibrium mixture of the three gases at 1150K contains 2.33×10^-2 M SO3(g) and 1.73×10^-2 M SO2, what is the equilibrium concentration of O2? ________ M (b) Consider the equilibrium system at 881 K. 2NH3 (g) --> N2 (g) + 3H2 (g) If an equilibrium mixture of the three gases at 881 K contains 6.06 x10^-5 M NH3,...
A.) Express the equilibrium constant for the combustion of ethane in the balanced chemical equation. 2C2H6(g)+7O2(g)⇌4CO2(g)+6H2O(g)...
A.) Express the equilibrium constant for the combustion of ethane in the balanced chemical equation. 2C2H6(g)+7O2(g)⇌4CO2(g)+6H2O(g) K=[C2H6]2[O2]7 / [CO2]4[H2O]6 K=[CO2]4 / [C2H6]2[O2]7 K=K=[CO2]4[H2O]6 / [C2H6]2[O2]7 K=[CO2][H2O] / [C2H6]2[O2] B.)Consider the chemical equation and equilibrium constant at 25∘C: H2(g)+I2(g)⇌2HI(g) , K=6.2×102 Calculate the equilibrium constant for the following reaction at 25∘C: HI(g)⇌12H2(g)+12I2(g) Express the equilibrium constant to two significant figures. C.) Consider the following reaction and corresponding value of Kc: H2(g)+Br2(g)⇌2HBr(g) , Kc=1.9×1019 at 25∘C What is the value of Kp...
part b. Determine the equilibrium constant, Kgoal, for the reaction 4PCl5(g)⇌P4(s)+10Cl2(g),    Kgoal=? by making use of the...
part b. Determine the equilibrium constant, Kgoal, for the reaction 4PCl5(g)⇌P4(s)+10Cl2(g),    Kgoal=? by making use of the following information: P4(s)+6Cl2(g)⇌4PCl3(g),       K1=2.00×1019 PCl5(g)⇌PCl3(g)+Cl2(g),       K2=1.13×10−2 Express your answer numerically.
3) A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10 atm ) and...
3) A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10 atm ) and O2(P= 1.10 atm ). When a catalyst is added the reaction 2SO2(g)+O2(g)⇌2SO3(g) takes place. At equilibrium the total pressure is 3.95 atm . Find the value of Kc. 4) Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.282 Mand [H2S]= 0.370 M . What is the value of the equilibrium constant (Kc)...
1. In which of the following reactions will Kc = Kp? A) 2 SO2(g) + O2(g)...
1. In which of the following reactions will Kc = Kp? A) 2 SO2(g) + O2(g) ⇌ 2 SO3(g) B) 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g) C) SO3(g) + NO(g) ⇌ SO2(g) + NO2(g) D) 2 N2(g) + O2(g) ⇌ 2 N2O(g) E) None of the above reactions have Kc = Kp 2. The reaction below has a Kp value of 3.3 × 10-5. What is the value of Kc for this reaction at 700...
The rate constant of a chemical reaction increased from 0.100 s−1 to 2.60 s−1 upon raising...
The rate constant of a chemical reaction increased from 0.100 s−1 to 2.60 s−1 upon raising the temperature from 25.0 ∘C to 45.0 ∘C . I solved (1T2−1T1) = −2.11×10−4   K−1 In (k1/k2) = -3.26 But, I'm having problems on this question: What is the activation energy of the reaction? Express your answer numerically in kilojoules per mole. It would be great if you could show all of your work. I've been trying to figure out this problem for a...
The equilibrium constant (Kc) for the following reaction is 6.7 × 10–10 at 630 °C. N2(s)...
The equilibrium constant (Kc) for the following reaction is 6.7 × 10–10 at 630 °C. N2(s) + O2(g) 2 NO(g) What is the equilibrium constant for the reaction below at the same temperature? 1/2 N2(g) + 1/2 O2(g) NO(g) a. 4.5 × 10−19 b. 3.4 × 10−10 c. 1.3 × 10−9 d. 1.8 × 10−5 e. 2.6 × 10−5
Assuming that each of the following reversible reactions has reached a state of equilibrium, indicate with...
Assuming that each of the following reversible reactions has reached a state of equilibrium, indicate with an arrow, showing direction of shift, the effect of each change upon the equilibrium. Assume that only one change is made at a time. a) 2 Cl2(g) + 2 H2O(g) + heat  4 HCl(g) + O2(g) (1) Raise P (2)Raise T b) Fe2O3(s) + 3 H2(g)  3 H2O(g) + 2 Fe(s) (1) Add Fe(s) (2) Raise P c) 2 NH3(g) + heat...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT