Time Altitude Pressure Temperature Volume Moles 9:00 pm 40 km 9.54 x 10 atm 115,580 L 9:10 pm 20 km 9.89 x 10° atm 25°C 117,860 L 1. Determine the temperature at 9:00 pm (Assume constant n). Show your solutions below. Justify your answer by providing an explanation of the process on how you were able to calculate the amount of gas.
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- A cylinder containing ethanol is submitted to a certain pressure. At a temperature of 273 K, when the applied pressure is 1.0 atm, the vapor pressure of the ethanol is 1.25 kPa. Considering that the molar volume of ethanol at 273 K is 1.22 x 10-2 dm3/mol, calculate the vapor pressure of ethanol when the pressure on the liquid reaches 4.00 MPa.Q1a-> A sample of hydrogen (H₂) gas was collected over water at 60°C. If the total volume of gas collected was 53.9 mL and the atmospheric pressure was 1.14 bar, what mass (in g) of hydrogen gas was collected above the water? The vapour pressure of water at 60°C is 150 torr. Q1b=> What is the molar mass (in g mol-¹) of a gas which has a density of 1.91 g/L at a pressure of 0.91 bar and temperature 15.3°C? Your answer may not correspond to an actual gas. Do not try to identify the gas.Melting point (Tm): -94.9C Boiling point (Tb): 110.7C a.) Using the data, find the vapor pressure of toluene at 20C in units of mol/L b.) What is the enthalpy of vaporization (∆?vap ) for toluene in kJ/mol?
- 3. A 12.0 cm3 sample of liquid H2O (density 1.00 g.cm-3) is heated to 328 oC under an external pressure of 0.8 atm, conditions under which it vapourises: (i) Calculate the volume of the gas. (ii) Calculate the mass of the same volume (as in part i) of CO2 gas under the same conditions. (iii) Calculate temperature of that sample of CO2 (as in part ii) at 8.0 atm pressure in a 20.0 L container.The table below shows temperature/composition data collected for a mixture of methylbenzene (M) and octane (O) at 1 atm. Recall that x stands for the mole fraction in the liquid and y stands for the mole fraction in the vapor in equilibrium. The boiling points for methylbenzene (M) and octane (O) are 110.60C and 125.60C, respectively. Construct the phase diagram with Temperature vs. xM. What is the composition of the vapor in equilibrium with the liquid of composition (a) xM = 0.250 and (b) xO = 0.250. T (0C) 110.9 112.0 114.0 115.8 117.3 119.0 121.1 123.0 xM 0.908 0.795 0.615 0.527 0.408 0.300 0.203 0.097 yM 0.923 0.836 0.698 0.624 0.527 0.410 0.297 0.164At 20.0°C, the vapor pressure of ethanol is 5.95 kPa, and at 63.5 °C, its vapor pressure is 53.3 kPa. Use this information to calculate the enthalpy of vaporization deltaHvap
- A sample of hydrogen (H2) gas was collected over water at 60°C. If the total volume of gas collected was 55.6 mL and the atmospheric pressure was 1.1 bar, what mass (in g) of hydrogen gas was collected above the water? The vapour pressure of water at 60°C is 150 torr. ..The vapour pressure of diethyl ether (C2H5OC2H5) at 25 °C is 545 mmHg. A closed 233 L drum contains 195 g of diethyl ether. The density of diethyl ether is 0.7133 g/ml. Approximately how many grams of diethyl ether in the container would be in the vapour phase at 25 °C? Round your final answer to three significant figures.solve as neatly as possible and show completesolution. Round your final answer to 4 decimal places and box / highlight all final answers. and all values must include proper units with proper conversion if needed in your solution. kindly folllow the format Given,Required,Solution subject physical chemistry 1. Calculate the mass of water vapor present in a room of volume 400 m3 thatcontains air at 290C when the relative humidity is 53.0%. Compute for the vaporpressure of water?
- Will liquid formaldehyde CH2O dissolve in ethanol CH3CH2OH? Draw a lewisstructure for both compounds. Then draw a diagram showing the the signand relative magnitude for each of the three parts of heat of solution. Be sureto indicate what kind of IMF is being broken or formed in each step. Use thisdiagram to support your conclusion.Argon makes up 0.93% by volume of air. Calculate its solu-bility (mol/L) in water at 20°C and 1.0 atm. The Henry’s lawconstant for Ar under these conditions is 1.5X10⁻³ mol/Latm.The standard enthalpy of vaporization of water, H2O, ΔvapH = 40.7 kJ/mol at 373 K. Assuming this value to remain constant at temperatures close to 373 K, use the Clausius-Clapeyron equation to estimate the vapor pressure of liquid water at 80°C.