Consider the following reaction at 1600ºC: Br2(g)  ⇌  2Br(g) When 1.05 moles of Br2 are put in a 0.980-L flask, 1.20 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction.

Consider the following reaction between nitrogen and oxygen and its equilibrium constant at 2000 °C: N2(g) + O2(g) ⇌ 2 NO(g)Kc = 4.10 × 10−4 a)Is the formation of nitrogen monoxide favored at 2000 °C? Explain your answer without doing a calculation. b)What is the nitrogen monoxide concentration when a mixture of 0.40 mol of nitrogen gas and 0.30 mol of oxygen gas reaches equilibrium in a 2.0-L container at 2000°C?

Consider the following reaction at 35oC:  N2O4(g) ⇌  2 NO2(g);  Kc=9.37 x 10-3. If the concentrations in the reaction mixture at some moment of time are: [N2O4] = 0.340 M, [NO2] = 5.33 x 10-2 M, then  the system is not at equilibrium and the reaction will proceed to the right the system is at equilibrium and no net change will occur the system is at equillibrium and the reaction will proceed to the left the system is at equilibrium and the reaction will proceed to the right the system is not at equillibrium and the reaction will proceed to the left

The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates: 4 NH3(g) +3 O2 (g) ⇌ 2 N2(g) + 6 H2O(g) When 0.0150 mol of NH3(g) and 0.0150 mol of O2(g) are placed in a 1.00−L container at a certain temperature, the N2 concentration at equilibrium is 1.96 ×10−3 M. Calculate Kc.

-2 The equilibrium constant K,, for the following reaction is 7.73×10atmat 350°C. What is the value of K. for the reaction at the same temperature? N2(g) +3H2(g)→ 2NH3(g)

Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0238 M, [N2] = 0.117 M, and [H2] = 0.347 M. Calculate Kc for the reaction at this temperature.

Consider the following chemical equilibrium: A(s) +  B(g) ⇄ 3 C(s) + 4 D(g) If the initial pressure of B is 4.26 bar, the total pressure at equilibrium is 7.15 bar. Use these pressures to calculate Keq.

Consider the following reaction and associated equilibrium constant at 430 K. 12 (g) + Br2 (g ) ⇌ 2 IBr (g) Kc = 278 If the reaction begins with 0.250 mol of IBr in a 2.00 L flask, calculate the concentration (mol/L) of IBr at equilibrium. Enter your answer with no units. Do not give handwriting solution.

For the reaction 2CO2 (g) ⇌ 2CO (g) + O2 (g), Kc = 6.4 x 10-7. If 1.0 x 10-3 moles of CO2 is placed in a 1.0 liter vessel, what are the concentrations of all species at equilibrium?

Initially, 2.0 moles of N2(g) and 4.0 moles of H2(g) were added to a 1.0-liter container and the reaction below then occurred. The equilibrium concentration of NH3(g) = 0.55 M at 700.°C. The value for Kc at 700.°C for the formation of ammonia is: 3H2(g) + N2(g) ⇌ 2NH3(g) a) 1.0 x 10^-1 b) 5.5 x 10^-2 c) 5.5 x 10^-3 d) 3.0 x 10^-1 e) The correct answer was not initially available