Suppose a 250. mL flask is filled with 0.90 mol of H,O, 1.2 mol of CO, and 1.5 mol of H,. The following reaction becomes possible: CO (g) + H,0(g) – Co,g)+H,(g) The equilibrium constant K for this reaction is 5.65 at the temperature of the flask. Calculate the equilibrium molarity of CO,. Round your answer to two decimal places. OM

When a reaction's reaction quotient is smaller than its equilibrium constant, what does this indicate about the reaction's equilibrium? The reaction must proceed in the reverse direction to return to equilibrium. The reaction is at equilibrium and will not change. O The reaction must proceed in the forward direction to return to equilibrium. O Nothing. There is no relationship between the reaction quotient and equilibrium constant.

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. = |

At a certain temperature, 0.3011 mol of N2 and 1.721 mol of H2 are placed in a 2.00 L container.   N2(g)+3H2(g)↽−−⇀2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, ?c.

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 1.5L flask with 2.9 atm of carbon monoxide gas and 2.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.4 atm of carbon monoxide gas, 1.4 atm of water vapor and 1.5 atm of carbon dioxide. The engineer then adds another 0.97 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 Submit Assignment Continue 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility MacBook Air DII 888 F10 F8 F9 esc F6 F7 F4 F5 F3 F2 %23 $4 % - & 4. 5 8.

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.

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.9 mol of NO,, 0.10 mol of N0 and 1.7 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 4.70 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M TRADIS Explanation Check 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Acces NOV 242 PAGES étv 4 MacBook Air II

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH,(g) = 3 H, (g) + C,H, (g) 8- = 2. × 10 He fills a reaction vessel at this temperature with 14. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H,, using only the tools yes x10 available to you within ALEKS? no ? If you said yes, then enter the equilibrium pressure of H, at right. atm Round your answer to 1 significant digit.

At a certain temperature, 0.88 mol N, and 2.654 mol H, are placed in a container. N2 (g) + 3H, (g) = 2NH; (g) At equilibrium, there is 0.82 mol NH, present. Determine the number of moles of N, and H, that are present when the reaction is at equilibrium. moles of N, at equilibrium: mol moles of H, at equilibrium: mol | privacy policy terms of use | help about us careers contact us O Ei A Gateway

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