At a certain temperature, the equilibrium constant K for the following reaction is 7.2 × 10-8: N₂(g) + O₂(g) 2 NO(g) Use this information to complete the following table. There will be very little N₂ and 0₂. Suppose a 7.0 L reaction vessel is filled with 0.97 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = -0 2 NO(g) N₂(g) + O₂(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 N₂(g) +20₂(g) 4 NO(g) x10

Nitrogen dioxide and carbon monoxide react to form nitrogen monoxide and carbon dioxide, like this: NO₂(g) + CO (g) →→ NO(g) + CO₂(g) - Use this chemical equation to answer the questions in the table below. Suppose 65.0 mmol of NO2 and 65.0 mmol of CO are added to an empty flask. How much NO₂ will be in the flask at equilibrium? 2 Suppose 215. mmol of NO and 215. mmol of CO₂ are added to an empty flask. How much NO₂ will be in the flask at equilibrium? O None. O Some, but less than 65.0 mmol. 65.0 mmol. More than 65.0 mmol. O None. O Some, but less than 215. mmol. ○ 215. mmol. More than 215. mmol.

Suppose a 500. mL flask is filled with 1.1 mol of NO2, 1.7 mol of NO and 0.90 mol of CO2. The following reaction becomes possible: NO, (g)+CO(g) NO(g) +CO,(s) The equilibrium constant K for this reaction is 0.292 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. м B C ol

The following reaction has an equilibrium constant of 1.94 x 10-10 at a certain temperature. COCl2(g)CO(g) + Cl2(g) If you have 0.93 moles of COCl2(g) in a 1.0L container, how many moles of CO will be present when the system reaches equilibrium?

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 2.0 mol of NO, and 1.3 mol of NO. The following reaction becomes possible: NO, (g) + NO(g) → 2NO, (g) The equilibrium constant K for this reaction is 6.91 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Explanation Check 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use |P 21

At a certain temperature, the equilibrium constant K for the following reaction is 0.0041: NO3(g) + NO(g) = ⇒2 NO₂(g) Use this information to complete the following table. There will be very little NO3 and NO. Suppose a 18. L reaction vessel is filled with 0.61 mol of NO₂. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO₂. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 NO2(g) P NO3(9) + NO (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 3 NO3(g) + 3NO(g) 6 NO₂(9) ܢܢ 3 ?

At a certain temperature, the equilibrium constant K for the following reaction is 0.54: NO,(g) + NO(g) 2 NO,(g) Use this information to complete the following table. 圖 Suppose a 36. L reaction vessel is filled with 0.97 mol of NO,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO3 and NO. x10 There will be very little NO2. ? olo Neither of the above is true. Ar What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 1.9 2 NO2(9) NO3(9)+NO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0.29 2 NO3(9)+2NO(9) 4 NO,(9) Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ........................................... ................ . .......... .........

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 1.1: Cl₂(g) + CHCl3(g) → HCl(g) + CCl4(g) Use this information to complete the following table. Suppose a 8.0 L reaction vessel is filled with 0.35 mol of HCI and 0.35 mol of CCl4. 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 2 significant digits. HCl(g)+CC1,(9) Cl₂(9)+CHC13 (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 3 Cl₂(g) + 3 CHCl3(g) P 3 HCl(g)+3CCI (9) There will be very little Cl₂ and CHCl3. There will be very little HCI and CCI4. Neither of the above is true. K = 0 K = 0 x10 X 5 olo 18 Ar U

Suppose a 500. mL flask is filled with 1.7 mol of OCl2, 0.70 mol of BrOCI and 1.1 mol of BrCl. The following reaction becomes possible: Br2(g) +OCl2(g) BrOCI(g) + BrCl (g) The equilibrium constant K for this reaction is 3.84 at the temperature of the flask. Calculate the equilibrium molarity of OCl2. Round your answer to two decimal places. ☐ M ☑

Calcium carbonate decomposes to form calcium oxide and carbon dioxide, like this: CaCO3(s) CaO(s) + CO₂(g) At a certain temperature, a chemist finds that a 2.8 L reaction vessel containing a mixture of calcium carbonate, calcium oxide, and carbon dioxide at equilibrium has the following composition: compound amount CaCO3 73.8 g CaO 42.1 g CO₂ 38.4 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = [0]