Calculate the actual pressure for a non-ideal system for 1.00 mole of carbon dioxide gas in 3.00 L at 0.00 oC with a = 3.59 L2·atm/mole2 and b = 0.0427 L/mole.
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Calculate the actual pressure for a non-ideal system for 1.00 mole of carbon dioxide gas in 3.00 L at 0.00 oC with a = 3.59 L2·atm/mole2 and b = 0.0427 L/mole.
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- 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.Calculate the actual pressure for a non-ideal system for 1.00 mole of carbon dioxide gas in 3.00 L at 0.00 oC with a = 3.59 L2·atm/mole2 and b = 0.0427 L/mole. Group of answer choices 7.44 atm 21.2 atm 6.38 atm 7.18 atm 19.1 atmIdeal Gas Law The pressure P, temperature T, and volume V ofan ideal gas are related by PV = nRT, where n is the number ofmoles of the gas and R is the universal gas constant. For the pur-poses of this exercise, let nR = 1; therefore, P = T/V.a. Suppose that the volume is held constant and the temperatureincreases by ∆T = 0.05. What is the approximate change inthe pressure? Does the pressure increase or decrease?b. Suppose that the temperature is held constant and the volumeincreases by ∆V = 0.1. What is the approximate change in thepressure? Does the pressure increase or decrease?c. Suppose that the pressure is held constant and the volume in-creases by ∆V = 0.1. What is the approximate change in thetemperature? Does the temperature increase or decrease?
- Pressure (A) Explain the term pressure and state its S.I. unit. (B) Explain Henry’s law. (C)A bottle of H2 has just been received by the technicians in DkIT for use in the instrumentation lab. It is a 47 litre cylinder at a pressure of 50 atmospheres. The normal working pressures is 2 bar. (i) To what volume of gas will that equate at the working pressure? (ii) For how many hours will the gas last if it used at the rate of 0.5dm3 per hour? D)You see your best friend at the bar and you walk up behind her. You accidentally startle her and she takes a step backwards. Unfortunately, she is wearing high heels and her heels come down on your foot. She weighs only 55kg but the size of her heel is 6mm by 6mm.Determine the pressure that she applies on your foot. (E) If a diver dives to a depth of 35 m what will be: (i) the pressure in Pascals due the water column? (3 marks) (ii) the pressure of the air in…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?(a) A rigid tank contains 1.60 moles of helium, which can be treated as an ideal gas, at a pressure of 28.0 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.00 atm. How many moles are removed? mol (b) What If? In a separate experiment beginning from the same initial conditions, including a temperature T, of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 28.0 atm to 5.00 atm. What is the final temperature (in °C) of the gas? °C
- Calculate the partial pressure of O2 produced from 1.80 L of 0.576 M N2O5 solution at 45 ∘C over a period of 20.8 h if the gas is collected in a 10.3-Lcontainer. (Assume that the products do not dissolve in chloroform.)3. (8pts) A mixture of three gasses, A, B, and C has a total pressure of 1.20 atm at 300 K. Calculate the partial pressure of each constituent knowing their respective amounts: na = 2.25 mol ; ne = 0.60 mol ; ne = 0.15 mol 4. (8pts) What would be the total pressure (in bar) of the mixture in question 3 if the gases were perfect and occupied a total volume of 1 L?What is the effect of the following on the volume of 1 mol of an ideal gas?(a) The pressure is reduced by a factor of 4 (at constant T).(b) The pressure changes from 760 torr to 202 kPa, and the temperature changes from 37°C to 155 K.(c) The temperature changes from 305 K to 32°C, and the pressure changes from 2 atm to 101 kPa.
- C6H12O6(aq)+ 2C2H5OH(aq)= 2CO2(g) Fermentation of 750 mL grape juice (density= 1.0g/L) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol . Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25 degrees Celcius? (The density of ethanol is 0.79g/L .)References Use the References to access important values if needed for this question. Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 754 mm Hg. If the wet H2 gas formed occupies a volume of 6.46 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °C. Submit AnswerA gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.
