In an experiment, 7.01 atm each of H2 and Cl2 were placed into a 1.00 L flask and allowed to react  H2(g)+Cl2(g)=2HCl(g) given that Kc=68.1, what is the equilibrium pressure of HCl

At a certain termperature, Kc = 0.914 for the reaction NO₂(g) + NO(g) = N₂O(g) + O₂(g) A mixture was prepared containing 0.200 mol NO2, 0.300 mol NO, 0.150 mol N₂O, and 0.250 mol O₂ in a 8.00 L container. What will be the equilibrium concentrations of each gas? [NO₂] [NO] [N₂O] [0₂] i i i i M M M M

For the equilibrium 2lBr(g) = 12(g) + Br2(g) Kc = 8.50 × 10³ at 150 °C. If 0.0600 mol of IBr is placed in a 1.0-L container, what is the partial pressure of I₂(g) in atm after equilibrium is reached?

A gaseous mixture contains 0.27 mol CO, 0.12 mol H2, and 0.022 mol H,O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. CO(9) + 3H, (9) = CH4 (9) + H,O(9) What is the concentration of CH4 in this mixture? The equilibrium constant K, equals 3.99.

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.

For the following reaction at a certain temperature, 1.57 mol H2 and 1.56 mol l2 are placed into a 2.05 L flask. At equilibrium, 2.70 mol of HI has been formed. Calculate Kc. H2(g) + 12(g) = 2 HI(g)

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N,(g) + 3 H,(g) 2 NH3(g) K = 1. × 10 He fills a reaction vessel at this temperature with 10. atm of nitrogen gas and 3.9 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes tools available to you within ALEKS? no ? If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.

A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining

A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp =

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N, (g) + 3 H, (g) = 2 NH3 (g) К, — 3. х 10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 3.2 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.