Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: Co (g) + H,O(g) – Co,g)+H,(g) The equilibrium constant K for this reaction is 0.735 the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -2 N2(g) + 3 H,(g) 2 NH3(g) K,=4. x 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 4.5 atm of hydrogen gas. Use this data to answer the questions in the table below. dla O yes Can you predict the equilibrium pressure of NH, using only the tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of NH, at right. ||atm Round your answer to 1 significant digit. Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Accessibility

General Chemistry 4th Edition McQuarrie Rock Gallogly University Science Books presented by Macmillan Learning For the chemical equation SO, (g) + NO, (g) = SO,(g) + NO(g) the equilibrium constant at a certain temperature is 2.10. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.64 mol SO, (g) in order to form 1.20 mol SO, (g) at equilibrium. 3 moles of NO,(g): mol 2. Question Source: MRG - General Chemistry | Publish privacy policy | help terms of use contact us about us careers (? ^ N EV prime video W

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 125. L tank with 11. mol of sulfur dioxide gas and 35. mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 7.7 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K. = |

Suppose a 500. mL flask is filled with 0.10 mol of NO,, 1.8 mol of NO and 0.50 mol of CO,. The following reaction becomes possible: 2' NO, (g) +CO(g) – NO(g) + CO, (g) The equilibrium constant K for this reaction is 1.08 at the temperature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. olo OM Ar G Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility .......................................... .................................

Suppose a 500. mL flask is filled with 0.70 mol of CO, 1.7 mol of NO and 1.0 mol of CO,. The following reaction becomes possible: NO, (g) +CO(g)- NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.97 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. IM Continue MacBook Air

Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(2)- -2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N2 O2 NO initial change equilibrium olo

Suppose a 500. mL flask is filled with 0.60 mol of CO, 0.30 mol of NO and 1.7 mol of CO,. The following reaction becomes possible: NO,(9) + CO(2) = No(g) + CO,(g) The equilibrium constant K for this reaction is 0.953 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. 0.37 M ?

Suppose a 500. mL flask is filled with 0.40 mol of N, and 0.10 mol of 0,. The following reaction becomes possible: N, (g) + 0,(g) – 2NO(g) The equilibrium constant K for this reaction is 5.29 at the temperature of the flask. Calculate the equilibrium molarity of N,. Round your answer to two decimal places. OM