2 H2S(g) + CH4(g) -> 4 H2(g) + CS2(g) Kc= 5.27 * 10-8 at 973 K Write the Kc expression for the equation above What is Kc for formation of one mole of H2S(g) at 973 K?
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1. 2 H2S(g) + CH4(g) -> 4 H2(g) + CS2(g)
Kc= 5.27 * 10-8 at 973 K
Write the Kc expression for the equation above
What is Kc for formation of one mole of H2S(g) at 973 K?
2.
H2((g) + O2(g) + C(graphite) -> HCHO(g) Δ H° f = -108.6 kJ mol-1
Write the Kp expression
What happens to the equilibria when the reaction temperature is increased ? Why ?
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- 42 Air is often dry air, ignoring the water mole fractions of in dry air 0.7808 and 0.2095, respectively. If the atmospheric pressure outside is 0.944 atm and the pressure associated with water is 0.039 atm, what are the partial of nitrogen and oxygen.A student obtains the following data by following an experimental procedure to this one. Based on this data, what is the value of R (in L.atm/mol/K) that would be calculated? Report the result to four significant figures. Use 273.15 K for the temperature conversion. Pressure of dry H2 = 742.0 mm Hg Temperature = 22.00 degrees C Mass of Mg used = 0.03860 g Volume of H2 = 44.10 ET units Conversion factor = 0.8119 mL/ET UnitCalculate ΔSvap for hydrogen sulfide from the following data: normal boiling point of H2S: -60.7oC ΔHvap of H2S: 18.7 kJ/mol Place ΔSvap in units of J/(mol K) and your answer should have 3 significant figures.
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- You have containers of pure O2 and N2 at 298 K and 1 atm pressure. You may assume the gases act like ideal gasses. Calculate ΔGmixing relative to the unmixed gases of: a) a mixture of 15 mol of O2 and 15 mol of N2. b) Calculate ΔGmixing if 12 mol of pure N2 are added to the mixture of 15 mol of N2 and 15 mol of O2. c) Calculate ΔSmixing for the system described in part b). d) Determine ΔHmixing for the system described in part b).Natural gas is very abundant in many Middle Eastern oilfields. However, the costs of shipping the gas to markets inother parts of the world are high because it is necessary toliquefy the gas, which is mainly methane and has a boilingpoint at atmospheric pressure of -164 °C. One possiblestrategy is to oxidize the methane to methanol, CH3OH,which has a boiling point of 65 °C and can therefore beshipped more readily. Suppose that 10.7 * 109 ft3 of methaneat atmospheric pressure and 25 °C is oxidized to methanol.(a) What volume of methanol is formed if the densityof CH3OH is 0.791 g>mL? (b) Write balanced chemicalequations for the oxidations of methane and methanol toCO21g2 and H2O1l2. Calculate the total enthalpy changefor complete combustion of the 10.7 * 109 ft3 of methanejust described and for complete combustion of the equivalentamount of methanol, as calculated in part (a).(c) Methane, when liquefied, has a density of 0.466 g>mL;the density of methanol at 25 °C is 0.791…Consider the complete combustion of glucose (C6H12O6) with O2 and calculate the moles of CO2produced when 1.02 g of glucose is reacted with 25 mL of O2 at body temperature (37 ºC) and 0.970 atm. C6H12O6 + 6 O2 (g) → 6 CO2 (g) + 6 H2O a. 0.95 b. 0.0022 c. 9.53 x 10-4 d. 6.33 x 10-2 e. 5.67 x 10-3
- For the following equation at 500 K, Kc = 7.9 x 1011.H2(g) + Br2(g) ⇌ 2 HBr(g) Find the Kc values for the following equations:a) 2 HBr(g) ⇌ H2(g) + Br2(g) Kc = ?b) 4 HBr(g) ⇌ 2 H2(g) + 2 Br2(g) Kc = ?A 10.0 g sample of liquid water is closed in a 1515 mL flask and allowed to reach equilibrium with its vapor at 27ºC. >What is the mass of H2O(g) when equilibrium is established? Data: Pv (H2O, 27ºC) = 26.7 torr.Carbon monoxide, a toxic product from the incomplete combustion of fossil fuels, reacts with water to form CO2 and H2, as shown in the equation CO(g) + H2O(g) ⇌ CO2(g) + H2(g), for which ΔH° = −41.0 kJ/mol and ΔS° = −42.3 J cal/(mol·K) at 25°C and 1 atm. What is ΔG if the gases have the following partial pressures: PCO = 1.3 atm, PH2O = 0.8 atm, PCO2 = 2.0 atm, and PH2 = 1.3 atm?