4) Balance the following reactions and convert them to their correct reaction quotients. Convert to either K. or Kp depending on what is given: a. NO2(g) + CO(g) E→ NO2(g) + CO2(g) + NO(g) b. Cl(ag) + 2 O2(ag) <→ clo, (ag) c. CHCI;(g) + HCI(g) → CH2CI2(g) + Cl2(g) Kc = 4.448 at 0°C Kp = 5.3x105 at 300°C K. = 0.000400 at -200°C %3D

For the equilibrium N2(g)+O2 <-->2NO(g), Kp = 0.0017 at 2300 K. At a given point, the partial pressures of the gases are PN2=PO2 = 0.660 atm and PNO= 0.0272atm. Which statment below is true? a. Q < K, so the reaction will continue to make more products. b. Q > K, so the reaction will consume products to make more reactants. c. Q = K, so the system is at equilibrium. d. The value of K will decrease until it is equal to Q. Show your work:

3. Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium: Keq = 4.6 × 10¹ a. A 1.00 L flask containing 0.0500 mol NO (g), 0.0155 mol Cl₂ (g), and 0.500 mol NOCI(g): 2NO(g) + Cl₂(g) = 2NOCI(g) A: shift right b. A 5.00 L flask containing 14 g N₂ (g), 12 g H₂ (g), and 17 g NH3(g): N₂(g) + 3H₂(g) = 2NH3(g) Keq = 0.060 (at 526 °C) c. A 2.00 L flask containing 230 g SO3 (8) 2SO3(g) = 2SO₂(g) + O₂(8) Keq = 0.230 A: shift left A: shift right

The value of K, for the reaction 2 NO, (g) N204 (g) is 1.52 at 319 K. What is the value of the Kp of the reaction NO2 (g) 1/2 N204 (g) at this temperature: 0.761 O2.31 1.23 1.52 0.811 A Moving to another question will save this response. Esc AI C 中 F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 23 %24

+60130 11. The reaction SbFs (g) + 4 Cl2 (g) SbCl3 (g) + 5 CIF (g) has an equilibrium constant of 0.02 at 300°C. Portions of the SbFs (g) and Cl2 (g) are mixed at 300°C and each have a partial pressure of 0.12 atm before the reaction. What is the reaction quotient, Q, before the reaction? b a. 0.02 d. 0.12 b. 1 e. 0 4/7 c. 2.5x10-5

In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC.  In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first.  This mixture is also heated to 350 oC.  After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas. PCl3(g) + Cl2(g)  PCl5(g). A gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibriate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.128 atm, PCl2 = 0.141 atm, and PPCl5 = 1.21 atm. (a) What is the value of Kp at this temperature? ______ (b) Does the equilibrium favor reactants or products? The equilibrium favors products. The equilibrium favors reactants.     Neither reactants nor products are favored.

3. Consider the reaction Br2 (g) + Cl2 (g) 2 BrCl (g) Kp = 1.11 x 104 at 150 K. A reaction mixture initially contains a Br2 partial pressure of 0.993 atm and a Cl2 partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO₂ (g) + H2 (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. CO (g) + H₂O (g) Kp = 0.0611 at 2000K.

2. Use the following information to calculate Kp and Ke for each reaction at 1000 K. CO2(g) + C(s) = 2C0(g) Kp = 1.50 at 1000 K a. 2c0(g) = CcO2(g) + C(s) 1 b. ½ CO2(g) + ½ C(s) = CO(g) c. 4C0(g) = 2CO2(g) + 2C(s)

Qq.1. Subject  :- Account