Natural gas is very abundant us many Middle Eastern oil fields. However, the costs of shipping the gas to markets in other parts of the world are high because it is necessary to liquefy the gas% which is mainly methane and has a boding point at atmospheric pressure of —164 °C. One possible strategy is to oxidize the methane to methanol. CH3OH. which has a boiling point of 63°C and can therefore be shipped more readily. Suppose that 10.7
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Chemistry: The Central Science, Books a la Carte Edition (13th Edition)
- On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm (STP) evolves 75.65 kJ of heat. If the gas is a mixture of ethane (C2H6) and propane (C3H8), what is the mole fraction of ethane in the mixture?arrow_forwardChlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the average molecular mass for this samplearrow_forwardChlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 1.43 g/L at 26 °C and 0.405 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of CH2F2 in the sample.arrow_forward
- Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111-trifluoroethane (C2H3F3) has a density of 2.39 g/L at 23 °C and 0.593 atm. 1. Calculate the average molecular mass for this sample. 2. Calculate the volume percentage of C2H3F3 in the sample.arrow_forwardChlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111- trifluoroethane ((C2H3F3) has a density of1.95 g/L at 23 °C and 0.432 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of C2H3F3 in the sample.arrow_forwardChlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 2.99 g/L at 22 °C and 0.810 atm. Calculate the average molecular mass for this sample.8.94×101 amu Calculate the volume percentage of CH2F2 in the sample.arrow_forward
- Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the volume percentage of CH2F2 in the sample.arrow_forwardNatural 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…arrow_forwardNatural 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 x 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 toCO2(g) and H2O(l). Calculate the total enthalpy changefor complete combustion of the 10.7 x 109 ft3 of methane just 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 g/mL.…arrow_forward
- For an ideal gas P= nRT/V, and for a gas whose molecules have volume P=nRT/(V-nb) How would you modify this latter equation for a real gas to correct for the fact that there are attractive forces between molecules.arrow_forwardIn the primary stage, a mixture of steam and methane at about 30 atm is heated over a nickel catalyst at 800°C to give hydrogen and carbon monoxide: CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g) ΔH°=260 kJ/mol The secondary stage is carried out at about 1000°C, in the presence of air, to convert the remaining methane to hydrogen: CH4 (g) + 1/2 O2 (g) ⇌ CO (g) + 2 H2 (g) ΔH°=35.7 kJ/mol (a) What conditions of temperature and pressure would favor the formation of products in both the primary and secondary stage? (b) The equilibrium constant Kc for the primary stage is 18 at 800°C. Calculate Kp for the reaction. (c) If the partial pressures of methane and steam were both 15 atm at the start, what are the pressures of all the gases at equilibrium? Thank you so much!arrow_forward(a) How much heat is released when 25.0 g of methaneburns in excess O₂ to form gaseous CO₂ and H₂O?(b) Calculate the temperature of the product mixture if themethane and air are both at an initial temperature of 0.0C.Assume a stoichiometric ratio of methane to oxygen from theair, with air being 21% O₂ by volume (c of CO₂=57.2 J/molK;c of H₂O(g)= 36.0 J/molK; c of N=230.5 J/molK).arrow_forward
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