The equilibrium constant K_eq for the reaction CO_2(g) rightarrow CO(g) + 1/2O_2

Question

The equilibrium constant K_eq for the reaction CO_2(g) rightarrow CO(g) + 1/2O_2(g) is 6.66 times 10^-12 at 1000 deg K. Calculate K for the reaction below: 2CO_2(g) + O_2(g) rightarrow 2CO_2(g) 2. The equilibrium constant, K_c, for the following reaction is 1.05 at 350 deg K. 2CH_2Cl_2(g) rightarrow CH_4(g) + CCl_4(g) If an equilibrium mixture of the three gases at 350 deg K contains 0.0206 M CH_2C_2(g), and 0.0163 M CH_4, what is the equilibrium concentration of CCl_4? 3. Methylamine, CH_3NH_2, is a weak base. CH_3NH_2(aq) + H_2O(l) rightarrow CH_3NH_3^+(aq) + OH^-_(aq) If the pH of a 0.065 M solution of the amine is 11.70, what is the value of K_b? 4. Calculate the pH of a solution that has an ammonium chloride concentration of 0.050 M and an ammonia concentration of 0.045M. 5. What is the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution consisting of 0.169 M NH_3 and 0.183 M NH_4Cl? 6. At 20 deg C, a saturated aqueous solution of silver acetate, AgCH_3CO_2, contains 1.0 gram of the silver compound dissolved in 100.0 mL of solution. Calculate the K_sp for silver acetate. AgCH_3CO_2(l) rightarrow Ag(aq) + CH_3CO_2(aq)

Explanation / Answer

1.The equilibrium constant K eq for the reaction CO2 --- > CO + ½ O2 is 6.66x10^-12 at 1000 deg K.

Calculate K for 2 CO(g) + O2(g) <-----> 2 CO2(g)

First calculate the K for the following reaction:

2 CO2 <--------> 2CO (g) + O 2 K = 6.66 x 10 ^ - 12 x 6.66 x 10 ^ - 12

K = 44.36 x 10 ^ - 24

Now reverse the above rreaction:

2CO (g) + O 2 ---- > 2 CO2 K 1/ K

K = 1/ 44.36 x 10 ^ - 24

K= 2.25 x 10 ^ - 22

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.