Please please just solve last two sub-parts (e and f) accurate and exact When it comes to gaseous substances, the concentration can be expressed as either a molarity value ora partial pressure value. The partial pressure for a gas can be determined using PV = nRT. (R = Gas lawconstant). When solving an equilibrium using a Kp value you must use the partial pressures of the gasesrather than the molarity. Complete the following problem using your knowledge of equilibrium andpartial pressures.The reaction of H2(g) and I2(g) to give HI(g) has an equilibrium constant, Ko, of 56 at 435°C.H2(g) + I2(g) = 2HI(g)A chemist mixes 0.45 mol of H2 and 0.45 mol of I2 in a 10.0 L flask at 435°C and allows thesystem to achieve equilibrium.What is the value of K,?а.b. Determine the initial partial pressure of H2 and I2. (Hint: PV = nRT)c. Complete the ICE box using the balanced equation and the partial pressure valuesdetermined in part b.d. Write the Kp expression for this equilibrium.Solve for the x value using the completed ICE box and the K, value determined in part a.Determine the equilibrium partial pressures of all species.е.f.

The given reaction is H2(g) + I2(g) <----> 2HI(g) ; Kc = 56 For the above reaction, change…

When it comes to gaseous substances, the concentration can be expressed as either a molarity value or a partial pressure value. The partial pressure for a gas can be determined using PV = nRT. (R = Gas law constant). When solving an equilibrium using a Kp value you must use the partial pressures of the gases rather than the molarity. Complete the following problem using your knowledge of equilibrium and partial pressures. The reaction of H2(g) and I2(g) to give HI(g) has an equilibrium constant, Ke, of 56 at 435°C. H2(g) + I2(g) = 2HI(g) A chemist mixes 0.45 mol of H2 and 0.45 mol of I2 in a 10.0 L flask at 435°C and allows the system to achieve equilibrium. a. What is the value of Kp? b. Determine the initial partial pressure of H2 and I2. (Hint: PV = nRT) c. Complete the ICE box using the balanced equation and the partial pressure values determined in part b. d. Write the Kp expression for this equilibrium. Solve for the x value using the completed ICE box and the K, value determined in part a. Determine the equilibrium partial pressures of all species. е. f.

When it comes to gaseous substances, the concentration can be expressed as either a molarity value or a partial pressure value. The partial pressure for a gas can be determined using PV = nRT. (R = Gas law constant). When solving an equilibrium using a Kp value you must use the partial pressures of the gases rather than the molarity. Complete the following problem using your knowledge of equilibrium and partial pressures. The reaction of H2(g) and I2(g) to give HI(g) has an equilibrium constant, Ke, of 56 at 435°C. H2(g) + I2(g) = 2HI(g) A chemist mixes 0.45 mol of H2 and 0.45 mol of I2 in a 10.0 L flask at 435°C and allows the system to achieve equilibrium. a. What is the value of Kp? b. Determine the initial partial pressure of H2 and I2. (Hint: PV = nRT) c. Complete the ICE box using the balanced equation and the partial pressure values determined in part b. d. Write the Kp expression for this equilibrium. Solve for the x value using the completed ICE box and the K, value determined in part a. Determine the equilibrium partial pressures of all species. е. f.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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