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)

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)

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...

See similar textbooks

Similar questions

Nitrogen dioxide decomposes according to the reaction 2 NO2 (g) ⇌ 2 NO (g) + O2 (g) Where Kp = 4.48 x 10 ^ -13 at a certain temperature. If 0.40 atm of NO is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO (g) and O2 (g)? P NO = atm NO P O2 = atm O2 Use correct significant figures.
What would be the equation for the following Kp expression: Kp= ( PHF) 2 I (PF2) (PH2)? H2 (g) = 2 HF (g) + F2 (g) 2F2 (g) + H2 (g) = 2 HF (g) O 2 HF (g) S H2 (g) + F2 (g) F2 (g) + H2 (g) = 2 HF (g)
For which of these reactions will there be no effect on the relative amounts of the substances present at equilibrium when the pressure of the system is increased at constant temperature? O 2 sO, (g) + 0,(g) = 2 SO, (g) + heat heat + CO, (g) + NO(g) =CO(g) + NO, (g) heat + 2 Cl, (g) + 2 H,O(g) = 4 HCI(g) + 0, (g) N, (g) + 3 H, (g) = 2 NH, (g) + heat
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.
If the exothermic reaction 2H2(g)+O2(g)→2H2O(g) has reached equilibrium, what is the effect of raising the temperature of the reaction vessel?
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.
Consider the reaction: Important values if I for this question C(s) + O₂(g) → CO₂(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: C(s) + 1/2O₂(g) → CO(g) K₁ CO(g)+1/2O,(g)=CO2(g) K2 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K =
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