1 (4 pts total) Consider the following equilibrium, for which Kp = 0.00154 at 500 °C: N: (e) 2 H,0 (e) 2 NO (E) 2 H; (e) Kp - 0.00154 a) (2 pts) What predominates at equilibrium, reactants or products? Why? Circle one: Reactants or Products Why? b) (2 pts) Calculate Kp for the reaction below. Use the original reaction above as reference: AN; (s) % H,O (e) +] % NO (e) A Hi (e)

1 (4 pts total) Consider the following equilibrium, for which Kp = 0.00154 at 500 °C: N: (e) 2 H,0 (e) 2 NO (E) 2 H; (e) Kp - 0.00154 a) (2 pts) What predominates at equilibrium, reactants or products? Why? Circle one: Reactants or Products Why? b) (2 pts) Calculate Kp for the reaction below. Use the original reaction above as reference: AN; (s) % H,O (e) +] % NO (e) A Hi (e)

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

10:25 1 4 7 +/- ||| For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25 °C, it is found that the partial pressure of C is 0.280 atm. What is AG° for this reaction? (R = 8.314 J/mol K). 2 5 Question 7 of 15 8 kJ/mol 6 9 * 10% 0 Submit Periodic Table X x 100
help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working
Consider the reaction: N₂O4 (9) 2NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: N2(g) + 202 (9) ⇒N₂O4(9) K₁ 1/2N₂(g) + O₂(g) NO₂ (g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K
As an environmental chemist you are studying formation of carbon monoxide, The following equilibrium constants were determine at 35°C:. (1) 2 C (s) + O2 (2) + 2 CO (2) Ke = 4.80 e-10 (2) 2 CO2 (e + 2 CO (g) + O2 (e) K = 1.10 e-5 i) Find Ke for CO2 1g) → C (s) + O2 (6) at 35°C ?
Consider the following equilibrium: 2NO () + Ci, e) - 2NOCI (e) AG--41. kJ Now suppose a reaction vessel is filled with 9.33 atm of chlorine (Ci,) and 6.96 atm of nitrosyl chloride (NOCI) at 481. "C. Answer the following questions about this system: O rise Under these conditions, will the pressure of Cl, tend to rise or fall? Is it possible to reverse this tendency by adding NO In other words, if you said the pressure of Cl, will tend to rise, can that be yes changed to a tendency to fall by adding NOr Similarly, you said the no pressure of Cl, will tend to fall, can that be changed to a tendency to me by adding NO If you said the tendency can be reverned in the second question, calculate the minimum pressure of NO needed to reverse it atm Round your arswer to 2 significant digits.
At 990◦C, Kc = 2.20 for the reaction:H2(g) + CO2(g) ⇀↽ H2O(g) + CO(g)How many moles of H2O(g) are presentin an equilibrium mixture resulting from theaddition of 1.19 mole of H2, 1.76 moles ofCO2, 0.974 moles of H2O, and 1.15 mole ofCO to a 5.00 liter container at 990◦C?1. 1.49 mol2. 1.40 mol3. 1.52 mol4. 1.43 mol5. 1.37 mol
Consider the reversible reaction A A B, with K = 0.1. Assume the reaction begins with only A, and draw a representation using molecular art for the reaction mixture at equilibrium. Use red spheres for A and blue spheres for B.
5
5. Kindly please provide the answer only ASAP
Please help with this
2. Explain how each of the following factors affects the amount of hydrogen gas present in an equilibrium mixture in the following reaction: 3 Fe(s) + 4 H,O(g) Fe;O4(s) + 4 H,(g) AH = - 150kJ a) raising the temperature of the mixture b) introducing more steam c) increasing the pressure
NetID: Name: 8. What is [NO] and [CO₂] (in M to two decimal places) at equilibrium for the following reaction at 227 °C if the initial concentrations of each reactant is 1.25 M? Explain the validity of your final answer using chemical intuition. NO₂(g) + CO(g) = NO(g) + CO₂(8) -224.09 kJ mol-1 K(227 °C) = 6.9x105 A: [NO] = 1.25; [CO₂] = 1.25