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- A gas mixture contains .923 g Ar and 1.25 g Br2 in a 4.0L vessel at 32C. Calculate the mole fraction, X, and partial pressure of each component in the mixture.A gas mixture at 300K and 200kPa consists of 1kg of CO2 and 3kg of CH4. Determine the partial pressure of each gasAt 100 kPa and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3H8) combusts, producing 18.0 g CO2 . Calculate the mole fraction of each gas in the initial mixture. Assume complete combustion.
- A flue gas contains 5 mole% H 2O. Calculate the ratios(a) kmol flue gas/kmol H 2O.(b) kmol dry flue gas/kmol flue gas.(c) kmol H 2 O/kmol dry flue gas.Underwater, the pressure increases by 1 bar for every 10 m of depth. When a scuba diver breathes pressurized air in which the partial pressure of N2(g) exceeds 4 bar, the result is nitrogen narcosis, which is similar to alcohol intoxication. What is the maximum mole percent of N2 in an air mixture that could be used by divers at depths up to 85 m below sea level without undue risk of nitrogen narcosis?100.0 g of propyne (C3H4) (g) is burnt in a 30.0 L rigid vessel containing pure O2 (g) at P = 10.00 bar and an initial temperature of 25.0 °C. At the end of the reaction the temperature of the vessel is 250. °C. At the end of the reaction, what are the partial pressures (in bar) of CO2 (g) and O2 (g)?
- If 15.1 g of the mixture with a volumetric composition of 45% N2, 35% O2 and 20% X gas is applying 3 atm pressure to a 5 dm3 volume vessel at 25 ° C, in which option is the molecular weight of X gas given correctly? (MN2: 28 gmol-1, MO2: 32 gmol-1)What is the mole fraction of magnesium nitrate, Mg(NO3)2, in an aqueous solution that is 5.549 wt % in magnesium nitrate? MW(Mg(NO3)2) = 148.315 g/mol. 5.834e-2 1.721e-1 7.080e-3 9.929e-1When zinc reacts with hydrochloric acid, zinc chloride and hydrogen gas are formed. After writing a balanced a equation, determine how many mL of 0.50 M HCl are required, with excess zinc, to produce 128 mL of hydrogen gas at 1.00 bar and 20.oC. Balanced equation: Zn + 2HCL --> ZnCl2 + H2
- What mass of C2H4 is needed to produce 56L of CO2(g) at 315k and 1.00ATM in a combustion reaction with excess oxygen gasConsider the following reaction CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) A mixture containing only CS2(g) and excess O2(g) at a total pressure of 100 kPa is placed in a sealed vessel. After the reaction is completed and the vessel is cooled to the initial temperature, the total pressure in the vessel drops to 80 kPa. What is the mole fraction of CO2(g) in the final mixture?A gaseous fuel contains by volume:CO2 = 2.6 % ,CO = 6 %, O2= O.6 % ,N2= 3.66 % ,H2= 48.0%CH4= 34 %, C2H4=5.2 %Calculate the minimum volume of air required for complete combustion of 100 m3 of the gas. If 50 % excess air is supplied, find the volume of each of the dry constituents of the flue gas.