Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3NO2(g) + H2O(l)-2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount K = NO2 10.6 g H₂O 138.4 g HNO3 21.8 g NO 19.6 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. x10 G

5.0 mole of ammonia were introduced into a 5.0L reaction chamber in which it is partially decomposed at high temperature. 2NH3(g)resulting 3H2(g)+N2 At equilibrium at a particular temperature, 80.0% of the ammonia had reacted. Calculate Kc(equilibrium constant) for the reaction.

Suppose a 250. mL flask is filled with 1.6 mol of Br₂, 0.70 mol of OC12 and 0.50 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrCl(g) The equilibrium constant K for this reaction is 2.87 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places. M Ś

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 924.: CO(g) + H₂O(g) → CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 17. L reaction vessel is filled with 0.75 mol of CO₂ and 0.75 mol of H₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. CO₂(g) + H₂(9) CO(g)+H₂O(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 CO(g) + 3H₂O(g) P 3 CO₂(g) + 3H₂(9) There will be very little CO and H₂O. There will be very little CO2 and H₂. Neither of the above is true. K = 0 K = 0 ■ x10 X ? 00. Ar 8.

Consider the following equilibrium. N2(s) + O2(g) 2 NO(g) At 2300 K, the equilibrium constant K - 1.7 x 10. Suppose that 0.015 mol NO(g), 0.16 mol N, (9), and 0.16 mol O, (9) are placed into a 10.0 L flask and heated to 2300 K. (a) Is the system at equilibrium? If the system is not at equilibrium, in which direction must the reaction proceed to reach equilibrium? The system is at equilibrium. OThe system is not at equilibrium. The reaction must proceed to the left. The system is not at equilibrium. The reaction must proceed to the right (b) Calculate the equilibrium concentrations of all three substances. (Enter unrounded answers.) [02 - [NO M

Suppose a 250. mL flask is filled with 1.1 mol of NO3 and 2.0 mol of NO. The following reaction becomes possible: NO3(g) + NO(g) → 2NO,(g) The equilibrium constant K for this reaction is 8.88 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.

A student ran the following reaction in the laboratory at 672 K: 2NH3(g)     N2(g) + 3H2(g) When she introduced 6.42×10-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 9.09×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 250. mL flask is filled with 1.8 mol of NO3 and 1.1 mol of NO2. The following reaction becomes possible: NO₂(g) + NO(g) + 2NO₂(g) The equilibrium constant K for this reaction is 0.707 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. M × S 1/5

A student ran the following reaction in the laboratory at 282 K: 2CH2C12(g)=CH4(g)+ CCI4(g) When she introduced 6.98x102 moles of CH,Ch(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62x10³ M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =