PCH. Construct the expression for Kp for the following reaction. CH₂(g) + CO₂(g) = 2 CO(g) + 2 H₂(g) Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. (Pco)² 2(PCH.) PH₂ Kp (PCH₂)² 2(PH₂) = Pco₂ 1 (PH₂)² 1 PCH₂ 2(Pco₂) (Pco₂)² Pco RESET 2(Pco)

Consider the hypothetical reaction A(g) 2B(g). A flask is charged with 0.74 atm of pure A. after which it is allowed to reach equilibrium at 0 °C. At equilibrium the partial pressure of A is 0.37 atm Part A What is the total pressure in the flask at equilibrium? Express your answer using two significant figures. VS ΑΣΦ 4 P₁ = Submit Part B What is the value of Kp? Express your answer using two significant figures. K₂= Submit Part C Request Answer |VL ΑΣΦ Submit Request Answer What could we do to maximize the yield of B? → Request Answer [w] ? O Doing the reaction in a larger flask maximizes the yield of B. O Doing the reaction in a smaller flask maximizes the yield of B. atm

5) At 25 °C the equilibrium constant of the reaction is Kel for the respective reactions and N₂(g) +3H₂(g) 2NH₂(g) (reaction 1) 3.5 x 108. What are the values Ke2 and Ke3 of the equilibrium constants = N2(g) +H₂(g) = NH₂(g) H₂(g) NH3(g), (reaction 2) 2NH3(9) N₂(g) + 3 H₂(g) 1 3 (reaction 3)?

Is this not 5.37?

Consider the following reaction where K. = 10.5 at 350 K: 2 CH2C12 (g) CH4 (g) + CCI4 (g) A reaction mixture was found to contain 1.23×10²² moles of CH,Cl, (g), 5.29×10² moles of CH4 (g), and 4.07×102 moles of CCl, (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: O 1. In order to reach equilibrium CH2CI,(g) must be consumed . O 2. In order to reach equilibrium K. must decrease . 3. In order to reach equilibrium CH, must be consumed . O 4. Qç is greater than K.. O 5. The reaction is at equilibrium. No further reaction will occur.

3. Given the chemical reaction A(aq) + 2B(aq) → C(aq) + 3D(aq) Initially, you have 2 moles of A and 3 moles of B dissolved in a total volume of 3 L. a. X moles of A reacted, and the solution reached equilibrium. Solve for the End state in term of x b. Write down the expression of the equilibrium constant (Keq) in term of x and volume.

In an experiment to study the formation of HI(g),H2(g) + I2(g) ⇌ 2 HI(g)At equilibrium, {H2} = 0.0137, {I2} = 0.0627 and {HI} = 0.0268. Calculate the value of Kc.

The reaction HCO₂H(g) CO(g) + H₂O(g) has Kp = 1.6 × 106 at 400 °C. What is the value of Kc for this reaction at this temperature? Kc = H

Consider the following chemical equilibrium: 4 NH; (g) + 3 0, (g) =2N, (g)+6H,0 (g) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator.