Suppose a 500. mL flask is filled with 1.3 mol of Cl,, 1.4 mol of HCl and 1.6 mol of CCl. The following reaction becomes possible: Cl, (g) + CHCI, (g) – HCI(g) +CC1, (g) The equilibrium constant K for this reaction is 0.723 at the temperature of the flask. Calculate the equilibrium molarity of CHCI,. Round your answer to two decimal places. OM

The equilibrium constant, K, for the following reaction is 6.30 at 723 K. 2NH3(g) ⇒N₂(g) + 3H₂(g) If an equilibrium mixture of the three gases in a 10.9 L container at 723 K contains 0.409 mol of NH3(g) and 0.291 mol of N₂, the equilibrium concentration of H₂ is M.

Suppose a 500. mL flask is filled with 1.2 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: Co(2) + H,0(g) – Co,(3) +H,(g) The equilibrium constant K for this reaction is 0.545 at the temperature of the flask. Calculate the equilibrium molarity of H,0. Round your answer to two decimal places.

References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant k for the following reaction is 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. 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 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)

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

Suppose a 500. mL flask is filled with 0.70 mol of Cl,, 1.4 mol of CHCI, and 0.50 mol of CCl,. The following reaction becomes possible: 3 Cl,(g)+ CHC1,(g) – HC1 (g)+ CCl,(g) 4 The equilibrium constant K for this reaction is 1.78 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. ||M

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

Calculating an equilibrium constant from a partial equilibrium.. 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 2.0 L flask with 3.9 atm of sulfur dioxide gas and 0.74 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.2 atm. Calculate the pressure 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, = [ %3D do x10 Ar Eplanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility FEB tv 23 30 MacBook Air DII DD F12 F11 F10 F9 80 888 F8 F7 F5 F6 F4 F3 esc F2 F1 $ % @ 8. 3 4 5 6 2 U

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