Problem #3 A given quantity of gas at a pressure of 750mmHg and a temperature of -25° C occupies 25L. What is its volume at STP? A. 269 B. 150L C. 27.1L D. 100L
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- A 200-cm3 vessel contains hydrogen gas at a temperatureof 25°C and a pressure of 0.990 atm. Unfortunately, thevessel has a tiny hole in its wall, and over a period of1 hour, the pressure drops to 0.989 atm. What is theradius of the hole (assumed to be circular)?How many grams of oxygen gas must be in a 10.0 L container to exert a pressure of 97.0 kPa at a temperature of 25oC? Show all work (Formalmethod).The pressure on 900 mL of a gas is 130 kPa. What must the pressure be changed to in order to make the volume 0.600L? (please show work)
- a tank used for filling helium balloons has a volume of 0.600m3 and conntains 3.00 mole of helium gas at 30.0o C. Assuminng that the helium behaves like an ideal gas, 1. What is the total translational kinetic energy of the molecules of the gas ? 2. Also using the fact that the molar mass of helium is 4x10-3kg/mole, determine the rms speed of the atoms at 20.0 of the atoms at 20.0oC.a) A certain sample of gas has a volume of 20.0 dm3 at 0oC and 1.0 atm. A plot of the experimental data of its volume against the celcius temperature, Ɵ, at constant pressure, gives a straight line of slope 0.074 dm3 /o From these data alone (without use of the perfect gas law) determine the absolute zero of temperature in degrees Celsius? b) Ballons are still used to deploy sensors that monitor meteorological phenomena. It is possible to investigate some of the technicalities of ballooning by using perfect gas law. Suppose your balloon has a radius of 3.0 m and that is spherical. What mass of H2 (in mol) is needed to inflate it to 1.0 atm in an ambient temperature of 25oC at sea level? What mass can the balloon lift at sea level,where the density of air is 1.22 kg /m3? What would be the payload if He were used instead of H2?Chemistry A certain gas obeys the Van der Waals equation with a = 0.500 Pa m6 mol-2, and with molar volume equal to 5.00 x 10-4 m3 mol-1 at 273.15 K and 3.00 MPa. (a) Calculate the value of the Van der Waals constant, b. (b) Calculate the value of the compression factor Z under these conditions. (c) Do attractive or repulsive forces dominate?
- A gas has a volume of 50.0L at 22 C. What will the volume be if it is cooled to -40 C? (please show work)Calculate the pressure exerted by 1.0 mol of hydrogen at 0oC in a vessel with volume of 5.0 dm3 using: a. The ideal gas law b. The Van der Waals equation (for constants see Table 1C.3, Resource section, p. 869) c. The Dieterici equation d. The virial EOS up to 2nd virial coefficient (use constant from Table 1C.1, p. 868) Book reference: Atkin's Physical Chemistry 11th Edition.....................An 85 g-mol gas 0ccupies 38 L at 78oC,,, wh@t is the vacuum pressure 0f the gas in psi??? CH0iceS: 210.4421 195.7421 -195.742 225.1421 961.6895 946.9895 932.2895 -932.289
- In Sample Exercise 10.16, we found that one mole of Cl2confined to 22.41 L at 0 °C deviated slightly from idealbehavior. Calculate the pressure exerted by 1.00 mol Cl2confined to a smaller volume, 5.00 L, at 25 °C. (a) First usethe ideal-gas equation and (b) then use the van der Waalsequation for your calculation. (Values for the van der Waalsconstants are given in Table 10.3.) (c) Why is the differencebetween the result for an ideal gas and that calculated usingthe van der Waals equation greater when the gas is confinedto 5.00 L compared to 22.4 L?How many moles of gas must be forced into a 3.1 LL ball to give it a gauge pressure of 8.4 psipsi at 23 ∘C∘C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.6 psipsi so that the total pressure in the ball is 23.0 psipsi .In a certain experiment, magnesium boride (Mg₃B₂) reactedwith acid to form a mixture of four boron hydrides (BₓHᵧ), threeas liquids (labeled I, II, and III) and one as a gas (IV).(a) When a 0.1000-g sample of each liquid was transferred to anevacuated 750.0-mL container and volatilized at 70.00C, sam-ple I had a pressure of 0.05951 atm; sample II, 0.07045 atm; and sample III, 0.05767 atm. What is the molar mass of each liquid?(b) Boron is 85.63% by mass in sample I, 81.10% in II, and 82.98% in III. What is the molecular formula of each sample?(c) Sample IV was found to be 78.14% boron. Its rate of effusion was compared to that of sulfur dioxide and under identicalconditions, 350.0 mL of sample IV effused in 12.00 min and250.0 mL of sulfur dioxide effused in 13.04 min. What is the mo-lecular formula of sample IV?