If PN₂,i = 0.79 atm and Pozi = 0.21 atm calculate the partial pressure of NO, N₂ and O₂ at equilibrium given K = 1 x 10-5. : 2 N₂(g) + O₂(g) → 2 NO(g)

At 30 degrees Celsius the Kc for 2CO(g) + O2(g) = 2CO2(g) is 2.24 x 1022. Predict in which direction the reaction will proceed to reach equilibrium, if we start with 55.0 g CO, 95.0 g O2 and 75.0 g CO2 in a 5.0 L vessel.

Consider the following reactions and their respective equilibrium constants: NO(g) + ½Br₂(g) = NOBr(g); K = 5.3 2NO(g) = N₂(g) + O₂(g); K = 2.1 × 10³⁰ Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N₂(g) + O2(g) + Br₂(g) = 2NOBr(g) Express your answer using two significant figures.

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.2 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.5 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = ☐ x10 ×

produces N20 and oxygen. Calculate the value of the equilibrium constant K. for the reaction 2 N,O4(g) –2 N,0(g) + 3 O2(g) from the following information: N2(g) + ¿O2(g) =N‚O(g) K¸ = 2.7 × 10-18 N,O4(g) =2 NO;(g) K. = 4.6 × 10-3 N2(g) + 2 O2(g) =2 NO2(g) K. = 1.7× 10-17

Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 2 NH3 (9) N₂H₁(g) + H₂ (9) Round your answer to 2 significant digits. K = 0 x10 x ⑤

Calculating an equilibrium constant from a partial equilibrium composition Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 2.0 L flask with 4.4 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 2.0 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = р x10 Ś ? olo 18 Ar B

The value of the equilibrium constant, Kc, for the following reaction is 0.13: A (g) + B (g) = C (g) + D (g) Calculate the value of Kc at the same temperature for the reaction 2A (g) +2B (g) = 2C (g) + 2D (g) a. 0.26 ○ a. O b. 3.8 × 10-2 О с. 0.15 d. 2.3 x 102 ○ d. ○ e. 1.7 x 10-2

Calculate the equilibrium partial pressure of H2

15.0 g of glucose reacts with oxygen in a 15.0 L container. At 250°C the system reaches equilibrium. At equilibrium it is determined that there are 5.25 mol of oxygen, 1.84 mol of carbon dioxide and 5.66 mol of steam. Calculate the value of the the equilibrium constant Kc. C6H12O6(s) + 602(g) = 6 CO2(g) + 6H2O(g) O9.64 x 10-5 O5.35 x 10 6 9- O1.87 x 105 O 0.0164 60.9