Q: Calculate the average molecular weight of air by mole fraction and mass fraction from its…
A: Mole fraction is ratio of the mole of the substance to the total no. Of moles present in the…
Q: Q4// A-Aclosed container of volume 0.02m contains a mixture of neon and argon at tempreture 27°c and…
A: Volume = 0.02 m3 Pressure = 1 × 105 Nm-2 Temperature = 27°C = 27 + 273 = 300 K Total mass of gases…
Q: n²a In the van der Waals equation, (P +) (v – nb) = nRT, explain why a term is added to %3D the…
A: Since you have posted multiple unrelated questions, we are entitled to answer the first only. a)…
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A: a). First we have to find the diameter of container, The volume of a spherical container V is given…
Q: What partial pressure of hydrogen results in a molarconcentration of 1.0 mmol dm3 in water at 25 oc?
A: Given data: Molarity of solution = 1 mmol/dm3 = 0.001 mol/L Temperature = 25oC Formula used:…
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Q: A vessel of volume 22.4 dm3 contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K. Calculate (a) their…
A: (a) According to unit conversion, 1 L is equivalent to 1 dm3. So, 22.4 dm3 is equivalent to 22.4 L.…
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A: VAN DER WAALS EQUATION: The Van der Waals equation for the real gases is given in the question. This…
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A: (a) Given data contains, Mass of argon is 25g. Volume is 1.5 dm3. Pressure is 2 bar. Temperature is…
Q: 4. A vessel of volume 0.2 m3 contains Nitrogen at 1,013 KPa and 15° C. If 0.2 kg Nitrogen is now…
A: Ideal gas eqation is general gas equation which obeys gas laws under all conditions of temperature…
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A: Formula of pressure: P = hdg Where h = height, d = density, g = acceleration due to gravity Given,…
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A: Given : Molar composition : % of CO2 = 30 % % of N2 = 40 % % of O2 = 100 - 30 - 40 = 70 %…
Q: Calculate the density of propane (C3H8) gas given p = 10° Pa and T = 273.15 K.
A: At STP one mole of gas occupies 22.4 L STP values: Pressure =105 Pa Temperature= 273.15 K d =m/v…
Q: Assuming that air may be treated as a mixture of ideal gases which has a mass composition 23.2%…
A: As per our guidelines we can only solve first question, please post other questions as next…
Q: Q4// A-Aclosed container of volume 0.02m° contains a mixture of neon and argon at tempreture 27°c…
A: Given : Volume = 0.02 m3 Temperature = 27°C Pressure = 1×105 Nm-2 Total mass = 28 g To find : Masses…
Q: At what pressure does the mean free path of argon at 20 °C become comparable to 10 times the…
A:
Q: A gas at 77.5 kPa and 17°C occupies a volume of 850cm^3, at what temperature in degrees Celsius…
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Q: At 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 L. In whichparts of the atmosphere…
A: Molar volume = 22.4 L
Q: Q2: Calculate the mole fraction of 15 % (w/w) C6H1206?
A:
Q: At what pressure does the mean free path of argon at 25 °c become comparable to the diameter of a…
A: T = 298 K λ= 1.0 dm3 = 0.1 m σ = 0.36 nm2 = 0.36 x 10-18 m2 λ=Rt2σP P=Rt2σλ
Q: 4. Consider a sample of gas at 393 K and 22 atm. (a) Calculate the molar volume V (L/mol) of the…
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Q: what is the temperature of .635 moles of neon in a 2.00L vessel at 4.68 degrees Celcius?
A: PV = nRT
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Q: 1.1(a) (a) Could 131 g of xenon gas in a vessel of volume 1.0 dm³ exert a pressure of 20 atm at 25°C…
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Q: Could 25 g of argon gas in a vessel of volume 1.5 dm3 exert a pressure of 2.0 bar at 30 °C if it…
A: The mass of the argon gas = 25 g The volume of the vessel = 1.5 dm3 The temperature of the gas = 30…
Q: What volume does 12.5 g of argon gas at a pressure of 1.05 atmand a temperature of 322 K occupy?…
A: Ideal gas equation The equation that gives the relationship between pressure, volume and temperature…
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Q: Q2: Calculate the mole fraction of 15 % (w/w) C6H12O6?
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Q: 1. (a) Could 131 g of xenon gas in a vessel of volume 1.0 dm 3 exert a pressure of 20 atm at 25°C if…
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Q: 1. Calculate the pressure(P) exerted by a 0.25 mole sulfur hexafluoride in a steel vessel having a…
A: 1. Given data: The number of moles of sulfur hexafluoride n=0.25 mol. The volume V=1.25 L.…
Q: 5.) The density of a gaseous compound was found to be 1.23 kg m3 at 330 K and 20 kPa. What is the…
A: Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: To what temperature must a sample of helium gas be cooled from 22.2 °c to reduce its volume from…
A: 1.00 dm3 = 1000 cm3 By Charles law : T2T1 =V2V1 T2(22.2 + 273.15) = 100 cm31000 cm3 T2 = 29.535 K…
Q: Calculate the mean speed of atoms of argon in a gas at 25 oC if the mean speed of neon under these…
A: (A)From the expression of root mean square velocity, it is clear that root mean square velocity of…
Q: At what pressure does the mean free path of Argon at 298 K become comparable to the size of a 1.000…
A: Given data,Temperature=298KDiameter=0.339nmwe know,1 nm=10-9mtherefore,0.339nm=0.339×10-9m
Q: n²a' In the van der Waals equation, (P +2) (V – nb) = nRT, explain why a term is added to the…
A:
Q: At 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 LIn which parts of the atmosphere…
A: Molar volume = 22.4 L
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A: Solution - Mass density - The mass density of an object is defined as its mass per unit volume. Mass…
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A: The ideal gas law is, PV=nRT The Van der Waal's equation of state is, (P+aV2)(V−b)=RT where, P is…
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- Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.Scottish physicist W. J. M. Rankine proposed an absolute temperature scale based on the Fahrenheit degree, now called degree Rankine abbreviated R and used by some engineering fields. If a degree Rankine is 5/9 of a degree Kelvin, what is the value of the ideal gas law constant in L. atm/mol. R?The Berthelot equation of state for one mole of gas is p=RTV-b-aTV2 Where a and b are constants determined experimentally. For NH3g, a = 741.6 atm. L2. K and b = 0.0139 L. Calculate p when V=22.41L and T = 273.15K. How much does the pressure vary from p as predicted by the ideal gas law?
- A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?What is the value of FP for a sample of gas whose temperature is -33.0 C and volume is 0.0250 L? What temperature is required to change the volume to 66.9 cm3?97 Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a new home. The propane gas consumed in 1.0 hour by a typical range burner at high power would occupy roughly 165 L at 25°C and 1.0 atm, and the range chosen by the client will have six burners. If the tank under consideration holds 500.0 gallons of liquid propane, what is the minimum number of hours it would take for the range to consume an entire tankful of propane? The density of liquid propane is 0.5077 kg/L.
- The gas in the discharge cell of a laser contains (in mole percent) 11% CO2, 5.3% N2, and 84% He. (a) What is the molar mass of this mixture? (b) Calculate the density of this gas mixture at 32C and 758 mm Hg. (c) What is the ratio of the density of this gas to that of air (MM=29.0g/mol)at the same conditions?The density of air 20 km above Earths surface is 92 g/m3. The pressure of the atmosphere is 42 mm Hg, and the temperature is 63 C. (a) What is the average molar mass of the atmosphere at this altitude? (b) If the atmosphere at this altitude consists of only O2 and N2, what is the mole fraction of each gas?Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
- In the anaerobic oxidation of glucose by yeast, CO2 is produced: If 1.56 L of CO2 were produced at 22.0 C and 0.965 atm, what mass of C6H12O6 is consumed by the yeast? Assume the ideal gas law applied.At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?