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27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction...
Question 26 6 pts 26. Consider the following chemical reaction: CO(g) + Cl2(8) -------------> COC12 (8) At the beginning 0.400 M CO(g) is mixed with 0.0500 M Cl2(g). At equilibrium, 0.0100 M of the product is produced. Calculate the equilibrium constant. OK -8.81 K-1.20 x 10exp-5 K=0.641 OK = 1.99x 10exp-3 Question 27 6 pts 27. Consider the following chemical reaction: N2(g) + 202(8) 2NO2(g) decreasing the pressure of reaction mixture will decrease amounts of O2(g) increase amounts of NO2(g)...
Calculate the value of the equilibrium constant for the reaction N2(g) + 2O2(g) ⇌ 2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0011, [O2] = 0.0033, and [NO2] = 0.0048. Keq = _______________
Consider the reaction N2(g) + 2O2(g) 2NO2(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER:
. Determine the value of the equilibrium constant for the reaction N2 (g) + 2O2 (g) ↔ N2O4 (g) from the following equations. ½ N2 (g) + ½ O2 (g) ↔ NO (g) KC = 6.9 x 10-16 2NO2 (g) ↔ 2NO (g) + O2 (g) KC = 4.5 x 10-13 2NO2 (g) ↔ N2O4 (g) KC = 6.7
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) Given the following reactions and enthalpies of formation: N2(g) + 2O2(g)→ 2NO2(g), ΔH∘ = 66.4kJ N2(g)+ O2(g)→ 2 NO(g), ΔH∘=180.4 kJ Please explain the steps as well!
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g)CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1530 M and a Cl2Cl2 concentration of 0.176 M at 1000 K. What is the equilibrium concentration of CO at 1000 K ? What is the equilibrium concentration of Cl2 at 1000 K ? What is the equilibrium concentration of COCl2 at 1000 K ?
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
Consider the following reaction: COCl2(g) -->CO(g) + Cl2(g) An equilibrium mixture of the three gases at 720 K contains 2.13×10-3 M COCl2, 3.16×10-2 M CO, and 2.71×10-2 M Cl2. What is the value of the equilbrium constant at 720 K? K =
Consider the following reaction at 350oC: N2(g) + 3 H2(g) ⇌ 2 NH3(g); Kc=70. If the concentrations in the reaction mixture at some moment of time are: [NH3] = 0.0100 M, [H2] = 0.0415 M and [N2] = 0.0200M , then Group of answer choices the system is at equilibrium and no net change will occur the system is not at equilibrium and the reaction will proceed to the left the system is at equilibrium and the reaction will proceed to...
Consider the equilibrium between COCl2, CO and Cl2. COCl2(g) CO(g) + Cl2(g) K = 0.112 at 904 K The reaction is allowed to reach equilibrium in a 7.00-L flask. At equilibrium, [COCl2] = 0.258 M, [CO] = 0.170 M and [Cl2] = 0.170 M. (a) The equilibrium mixture is transferred to a 14.0-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a...