4. a) If the initial partial pressures are PNO = 126, PNOBr = 275 torr, find...
4. Consider the reaction: 2 NO(g) + Br2 (g) 2 NOB (g) Kp = 31.8 at 302 K a) If the initial partial pressures are Pro = 108 torr, Per; = 126 torr, ProBr = 275 torr, find Qp and determine which direction the reaction proceeds in to reach equilibrium. 139.17 b) When a mixture of NO, Bra, and H, reaches equilibrium at 302 K, Pno=133 torr and Pers 151 torr. Find PNobr (in torr). [335 torr] 5. lodine gas...
In a gas mixture, the partial pressures are: CH 4 76.0 torr, He 230. mmHg, and N 2 0.640 atm. The total pressure in mmHg is ?
Review Topics] Use the References to access important values if needed for this question. ? The equilibrium constant, Kp for the following reaction is 1.80x10-2 at 698 K: 2HI(g) H2(g) +12(g) a eq Calculate the equilibrium partial pressures of all species when HI(g) is introduced into an evacuated flask at a pressure of 1.23 atm at 698 K. eg = atm PHI PH₂ P1₂ atm atm M Submit Answer Ratry Entire Group 2 more group attempts remaining Use the References...
Question 1. Phosphorous trichloride reacts with chlorine to produce phosphorus pentachloride: PC13(g) + Cl2(8) - PC1s(8) The equilibrium constant (Kc) for the reaction is 96 at 400 K If the equilibrium concentration of PC13 is 0.50 M and Cl, is 0.070 M, what is the equilibrium concentration of PCI ? Question 2. Consider the reaction between hydrogen and iodine H2(g) + 12(6) 2 HI(g) Kc = 64 Initially, a container was charged with 0.55 atm of H, and I2, what...
2. Convert K, based on concentration, to Kp, based on partial pressures. The term Δn means the number of moles of gas in the products minus the number of moles of gas in the reactants. Ifдп-0, K-Kp. An Kp K(RT) volume, at 250°C. a First calculate the moles of each gas present at equilibrium. 3 Calculate the partial pressures of N2, H2 and NH3 assuming a 10.0 L mol N2- mol H2 = mol NH3 b) Now find the total...
answer all questions for rating. 1. Part A Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 453 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.800 Cl2 1.24 COCl2 0.240 What...
Part A Phosgene (carbonyl chloride), COCl, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl2(g) =COC12(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 472 °C. At equilibrium, the concentrations were measured and the following results obtained: Partial Pressure Gas (atm) 0.890 Cl COCI 0.280 СО 1.26 What is the equilibrium constant,...
Please answer & explain 36-40 Calculate the volume of H2(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCI (g) solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. 2 HCl (g) + Mg(s) → MgCl2 (s) + H2(g) a) 0.56 L b) 4.47 L c) 2.23 L d) 1.12 L 37. What is the total pressure in atmospheres in a 10.0 L vessel containing 2.50 x 10-3...
Please answer all six thanks 1) The equilibrium constant for the following reaction is 2.90×10-2 at 1.15×103K. 2SO3(g) ------------------->2SO2(g) + O2(g) If an equilibrium mixture of the three gases in a 17.3 L container at 1.15×103K contains 0.437 mol of SO3(g) and 0.422 mol of SO2, the equilibrium concentration of O2 is M. 2) A student ran the following reaction in the laboratory at 1100 K: 2SO3(g) -------------------->2SO2(g) + O2(g) When she introduced 7.74×10-2 moles of SO3(g) into a 1.00 liter...
QUESTION 1 What does “ICE” stand for, with respect to chemical reactions? Immigration and Customs Enforcement In Case of Emergency Initial, Change, End Initial, Change, Equilibrium None of the above 1 points QUESTION 2 It is possible to solve for the value of K (the equilibrium constant) when: the equilibrium concentrations of all reactants and products are known. only the initial concentrations are known. the initial concentrations of the reactants and the equilibrium concentrations of one or more products are...