information to complete the following table. Suppose a 47. L reaction vessel is filled with 0.56 mol of NO₂ and 0.56 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. NO(g) + CO₂(g) NO₂(g)+CO(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits.

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.

At a certain temperature, the equilibrium constant K for the following reaction is 0.0087: NO₂(g) + CO(g) → NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 29. L reaction vessel is filled with 0.27 mol of NO₂ and 0.27 mol of CO. 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. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(g)+2CO(g) 2NO(g)+2CO₂(g) There will be very little NO₂ and Co. There will be very little NO and CO₂. Neither of the above is true. K = 0 0 0 x10 X ?

For the chemical equation: SO2(g) + NO2(g) SO3(g) + NO(g) The equilibrium constant at a certain temperature is 8.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 6.20 mol SO2(g) in order to form 4.40 mol SO3(g) at equilibrium.

Coal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gas

Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO2(g)→CaCO3(s) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount Cao 31.2 g CO2 16.8 g CACO3 32.3 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K = [| Submit A Continue MacBook Air F10

For the chemical equation 2SO2(g) + NO2(g) 2SO3(g) + NO(g) The equilibrium constant at a certain temperature is 5.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 1.20 mol SO2(g) in order to form 0.80 mol SO3(g) at equilibrium.

Consider the following reaction at equilibrium. What effect will removing some SO2 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The pressure of SO3 will increase The equilibrium constant will decrease. No change will occur since SO2 is not included in the equilibrium expression. The pressure of NO2 will increase. The reaction will shift to decrease the pressure.

For the chemical equation SO, (g) + NO, (g) = So, (g) + NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.75 mol SO,(g) in order to form 1.10 mol SO, (g) at equilibrium. moles of NO,(g): mol

When 0.16 mol of O2 gas and excess graphite were placed in a 2.00-L container and come to equilibrium, the concentration of CO gas was 0.088 0.024 M. What is the equilibrium constant, Kc, for this reaction at this temperature? Please report 4 decimal places, without units. C(s) + O2(g) ⟷ 2CO(g)