At 100 °C, Keg = 1.5E8 for the reaction: CO(g) + Cl2(g) - COCI2(g) Using appropriate approximation, calculate the partial pressure of CO at 100 °C at equilibrium in a chamber that initially contains COCI2 at a pressure of 0.292 bar. i bar

The partial equilibrium pressures for N2, O2, and NO in the reaction: N2(g) + O2(g) 2NO(g) are P(N2) = 0.25 atm, and P(O2) = 0.198 atm, and P(NO) = 0.050 atm.

A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established:   1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g)Peq   the equilibrium partial pressures of CH4, H2S, CS2, and H2. (CH4) =  7.5Peq(H2S) = 5.35Peq(CS2) = 6.42Peq(H2) =   1.5195   At equilibrium 0.01420 mol of H2 is found in the reaction mixture. Calculate KP for this reaction.KP = _____  .

For the reaction CuS(s) + O2(g) = Cu(s) + SO2(g), at equilibrium it is found that the partial pressure of SO, is 0.102 atm. If the reaction vessel has a volume of 0.250 L, and the temperature is 25 °C, how many moles of SO2 was produced? O 1.24x10-2 mol O 1.03x10-5 mol O 0.959 mol O 1.03x10-2 mol O 1.04x10-3 mol

Subject- chemistry

c. In a different equilibrium mixture, under different conditions, the partial pressures of the gases are shown in the table: Gas Partial pressure / kPa N2 1.20 x 102 H2 1.50 x 102 NH3 1.10 x 103 Calculate the value of the equilibrium constant (Kp) for this reaction and give its units. d. The enthalpy change for the reaction is -92 kJ mol-1 State the effect, if any, of an increase in temperature on the value of Kp for this reaction. Explain your answer. 3. a. Name the catalyst used in the Haber process. b. Explain why a catalyst does not change the yield of ammonia produced. c. Sketch a Maxwell Boltzmann distribution curve (with labelled axes) and use it to explain why a catalyst will increase the rate of reaction.

An evacuated (i.e. empty) vessel is charged with 0.0234 atm of 12 (g), 0.0234 atm of Br2 (g), and 0.6842 atm of IBr. The following reaction proceeds to reach equilibrium. 12 (g) + Br2 (g) = 2 1Br (g) The equilibrium constant for this reaction at this temperature is Kp = 247. At equilibrium, the pressure bromine gas in this system is ? atm. Report your answer to 3 significant figures, i.e. 0.0123 atm.

At 25.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) is at equilibrium when PCO2 = 3.50 mbar, [H2O] = 55.5 mol L-1, [H+] = 39.8 µmol L-1, and [HCO3-] = 1.28 mmol L-1. Then an additional 4.00 mbar of CO2 is added to the system. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1)

The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl₂(g) 80 F3 [CO] [Cl₂] Calculate the equilibrium concentrations of reactant and products when 0.245 moles of Co and 0.245 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K. = [COCI₂] = = $ 4 Use the References to access important values if needed for this question. Submit Answer NOV 30 Q ? An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. F4 CoCl₂(g). % 5 M M M Retry Entire Group 16 F5 tv ♫ 9 A 6 9 more group attempts remaining MacBook Air C F6 & 7 F7 * 8 DII F8 9 Previous Email Instructor F9 ) - O Next Save and Exit 4 F10 I

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