The following equilibrium constants were determine at 2400K: HI(g) → H2(g) + 12 (s) H(g) → H2(g) 12 (s) → (8) Kc = Kp = 6.71e-4 = 3.38e10 = Kp = i) Find K, for: HI(g) → H(g) + (g) at 2400 K? Kp = 3.00e-2 Use correct number of significant figures but no units. Use the format 6.02e-6 ii) If 1.00 mg of H, I and HI are placed in a 10.0L vessel at 2400K, what is Q Use correct number of significant figures but no units. Use the format 6.02e-6 iii) what direction will the reaction proceed? L = Left, R = Right, NC = No change Reaction shift = Type, L, R or NC

The following equilibrium constants were determine at 2400K: HI(g) → H2(g) + 12 (s) H(g) → H2(g) 12 (s) → (8) Kc = Kp = 6.71e-4 = 3.38e10 = Kp = i) Find K, for: HI(g) → H(g) + (g) at 2400 K? Kp = 3.00e-2 Use correct number of significant figures but no units. Use the format 6.02e-6 ii) If 1.00 mg of H, I and HI are placed in a 10.0L vessel at 2400K, what is Q Use correct number of significant figures but no units. Use the format 6.02e-6 iii) what direction will the reaction proceed? L = Left, R = Right, NC = No change Reaction shift = Type, L, R or NC

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

Given: C (s) + H2O(g) -> CO(g) + H2(g) Kp=1.6x10-21 at 298 If at 298 K PCO= 1x10-8 atm PH2= 2x10-4 atm PH2O= 5x10-5 atm and mass of C = 2g Is the mixture of gases at equilibrium ? Show your calculations. ( need to calculate Qp then compare ) If not, which direction will the reaction proceed to reach equilibrium?
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
2HOCI(g) ⇒ H₂O(g) + Cl₂O(g) Kp = 11.1 @ 298 K The reaction begins with 2.5 atm of HOCI, 0.5 atm H₂O, and 1.0 atm Cl2O. Calculate the equilibrium pressures of the components. What is the equilibrium pressure of HOCI? Рносі = ?] atm
Give proper explanation
SO₂(g) + Cl₂(g) = SO₂Cl₂(g) ΔΗ° = −264 kJ K = 34.5 When the reaction is altered, as below, what is the value of the new equilibrium constant? 3SO₂(g) + 3Cl₂(g) = 3SO₂Cl₂(g) K' = [?] К' Enter
Use the information below to complete the chart about Le Chateliers principle
Consider the reactions and their respective equilbrium constants: NO(g) + 1/2BR(g) > NOBR(g) KP = 5.3 2NO(g) > N2(g) + O2(g) KP = 2.1 x 1030 Use these reactions and their equilbrium constants to predict the equlibrium constant for the following reaction: N2(g) + O2(g) + Br2(g) > 2NOBR(g)
Nitric oxide reacts with chlorine to form NOCI. 2NO(g) + Cl2g) → 2NOCI(g) The equilibrium constant K at 298K is x 107. (R = 8.314 J/K • mol) Substance: NO(g) Cl2g) NOCIG) AH°F (k]/mol) at 298 K 90.29 51.71 S°U/K• mol) at 298 K 210.65 223.0 261.60
Equilibrium: 7. Write the equilibrium expression, K, for the following reactions: 2NH, (g) + CO2 (g) N,CH,0 (s) + H,0 (g) K= N2 (g) + 02 (g) 2 NO (g) K= 8. Consider the following reaction at equilibrium. 2S0, (g) 2S0, (g) + 02 (g) Predict the affect on equilibrium (will it shift left, shift right or no change?): a. Oxygen gas is removed: b. The volume is increased: c. The pressure is increased: d. SO, is added: e. SO, is added:
Picture
3. Consider the following reaction: XO(s) + CO(g) = X(s) + CO2(g) Kp = 0.403 at 100. °C At 100. 'C, the system is at equilibrium in a 1.00 L vessel and contains 1.00 moles of XO, 1.00 moles of CO, 0.403 moles of X, and 0.403 moles of CO2. a. Consider a case where all moles of X are removed from the system described above (volume and temperature remain constant). After waiting for the system to reach a constant composition, how many moles of CO2 will be present? b. Consider a case where all moles of CO are removed from the system described above (volume and temperature remain constant). After waiting for the system to reach a constant composition, how many moles of CO2 will be present?
A sample of NO decomposes according to the following equation: 2 NO(g) 1 N₂(g) + 1 0₂(9) An equilibrium mixture in a 10-L vessel at 8529 °C, contains 0.00354 g of NO, 0.00283 g of N₂, and 0.00266 g of 0₂. (a) Calculate Kp for this reaction at this temperature. Kp = = (b) What is the total pressure exerted by the equilibrium mixture of gases? Ptotal = atm.