Use the References to access important values if needed for this question. Consider the following reaction: 2HI(g) H2(9) + I2(g) If 3.49 moles of HI(g), 0.660 moles of H2, and 0.392 moles of I2 are at equilibrium in a 18.3 L container at 768 K, the value of the equilibrium constant, Ke, is Submit Answer Retry Entire Group 1 more group attempt remaining

Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 1.22×10-2 moles of COCl2(g), 0.591 moles of CO, and 0.561 moles of Cl2 are at equilibrium in a 15.3 L container at 789 K, the value of the equilibrium constant, Kc, is

Suppose a 500. mL flask is filled with 0.80 mol of H, and 0.90 mol of HI. The following reaction becomes possible: H, (g) +1,(g) – 2HI(g) The equilibrium constant K for this reaction is 3.50 at the temperature of the flask. Calculate the equilibrium molarity of I,. Round your answer to two decimal places. ?

Phosphorous pentachloride decomposes according to the reaction PCI, (g) PCI, (g) + Cl₂(g) A 12.3 g sample of PCI, is added to a sealed 1.50 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 33.6% of the PCI, remains. What is the equilibrium constant, K., for the reaction? Ke 0.0604 Incorrect

A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant.   A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont

Consider the following reaction: 2HI(g) = H2 (g) + I2 (g)   If 2.99 moles of HI(g) , 0.359 moles of H2, and 0.628 moles of I2 are at equilibrium in a 19.6 L container at 859 K, the value of the equilibrium constant, Kc , is .

Subject: chemistry

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

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.

Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is