Suppose a limekiln of volume 750. L is pressurized with carbon dioxide gas to 10.8 atm, and heated to 1140. °C. When the amount of CO, has stopped 2 changing, it is found that 2.59 kg of CaCO, have appeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaC0, and CaO at 1140. °C. Round your answer to 2 significant digits.

ating UP bunE Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquld form It is easily transported. An Industrial chemist studying this reaction fills a 200. mL flask with 1.6 atm of ammonia gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.7 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = Check Explanation 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility M 9 hp esc

9.Suppose 1.000 mole of CO and 3.000 mol of Hydrogen are put in a 10.000 L vessel at 1200 K. Determine the equilibrium composition of the reaction mixture if K. = 3.92 for the reaction. CO (g) + 3H₂(g) → CH4(g) + H₂O(g)

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S,(g) + C(s) = CS, (g) K. = 9.40 at 900 K How many grams of CS, (g) can be prepared by heating 13.0 mol S,(g) with excess carbon in a 5.70 L reaction vessel held at 900 K until equilibrium is attained? mass of CS,(g):

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 flask is filled with of and of . The following reaction becomes possible: The equilibrium constant for this reaction is at the temperature of the flask. Calculate the equilibrium molarity of . Round your answer to two decimal places.

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 4.6 atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.8 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.

For the equilibrium reaction.   2IBr (g) I2 (g) + Br2 (g) Kc=.0085.  If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components.   Consider the decomposition reaction at 555 K   4POCl3 (g)    P4  (g) + 2O2  (g) + 6Cl2  (g)   If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm.  Find Kp and Kc.

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 2.0 L flask with 3.7 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.74 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 = 0 P X S

At a certain temperature, 0.760 mol SO, is placed in a 2.50 L container. 2 SO,(g) = 2 SO2(g) + O,(g) At equilibrium, 0.120 mol O, is present. Calculate K.. Ke