4.(A) Indicate following statements as True (T) or False (F):(a) Higher the molar mass of a gas, faster its diffusion is.(b) Graham's law states that the rate of diffusion or effusion of a gas is inverselyproportional to the square root of its molar mass.(c) When NH3(g) and HCI(g) react to form NH,Cl(s), a blue precipitate is observed.(d) Diffusion is the process whereby gaseous atoms and molecules are transferred fromregions of relatively low concentration to regions of relatively high concentration.(e) The diffusion rate of a gas depends on the increase or decrease in concentration fromone point to another (concentration gradient), the amount of surface area available fordiffusion, and the distance the gas particles must travel.(B) If CH4(g) and C4HS(g) are released simultaneously at the left and right ends of a glass tubewith 50 cm length, respectively, at what distance from the left end of the tube will they meet?(CH4: 16 g/mol, C4H8: 56 g/mol)50 cmCH,-- CH,

The question is based on the concept of ideal gas. We have to identify the correct or incorrect…

4. (A) Indicate following statements as True (T) or False (F): (a) Higher the molar mass of a gas, faster its diffusion is. (b) Graham's law states that the rate of diffusion or effusion of a gas is inversely proportional to the square root of its molar mass. (c) When NH3(g) and HCI(g) react to form NH,CI(s), a blue precipitate is observed. ..... ........ .... (d) Diffua

4. (A) Indicate following statements as True (T) or False (F): (a) Higher the molar mass of a gas, faster its diffusion is. (b) Graham's law states that the rate of diffusion or effusion of a gas is inversely proportional to the square root of its molar mass. (c) When NH3(g) and HCI(g) react to form NH,CI(s), a blue precipitate is observed. ..... ........ .... (d) Diffua

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

(a) Which will effuse through a hole faster, bromine Br2(g) (molar mass: 159.8 g/mol) or C(CH3)4(g) (molar mass: 72 g/mol)? Why?(b) How much faster does one gas effuse faster than the other? Provide a numerical value
Decide whether each one of the following statement is correct, not correct, or conditionally correct. Justify your answers in each case. (a) As the pressure increases, a gas molecule travels a shorter distance before it collides with a neighbor. (b) Mean free path of a benzene molecule is larger than that of He.
At 287 K and 1.43*10^-2 atm, the density of a gas is 1.37*10^-5 g/cm^3. (a) Find the Vrms for the gas molecules. (b) Find the molar mass of the gas.
2. A sample of vapor weighing 0.368 g filled a Florence flask when heated in a water bath at 95.0°C. The actual volume of the flask was 128.4 mL and the barometric pressure was 747 torr. Calculate (a) the volume of the vapor at STP and (b) the molar mass of the volatile liquid. (Use the approach applied in the Introduction and on the data sheet.)
The partial pressure of water vapor in saturated air at 34 °C is 5.25×10-2 atm. (a) How many molecules of water are in 1.16 cm3 of saturated air at 34 °C? (b) What volume of saturated air at 34 °C contains 0.563 mol of water?
Because of their different molar masses, H₂ and D₂ effuse at different rates . (a) If it takes 16.5 min for 0.10 mol of H₂ to effuse, how long does it take for 0.10 mol of D₂ to do so in the same apparatus at the same T and P? (b) Howmany effusion steps does it take to separate an equimolar mix-ture of D₂ and H₂ to 99 mol % purity?
A gaseous “CFC” compound has a density of 5.456 g/L at 0.993 atmand 22.0oC. (a) Calculate the molar mass of the compound. (b) If the compound has the following composition: 18.10% C; 28.60% F, and 53.30% Cl, by mass, determine the molecular formula of the compound. (CFC = chlorofluorocarbon)
(1) (a) A sample of xenon gas at a pressure of 865 mm Hg and a temperature of 36 °C, occupies a volume of 11.9 liters. If the gas is heated at constant pressure to a temperature of 84 °C, the volume of the gas sample will be L. (b) A helium-filled weather balloon has a volume of 525 L at 22.9°C and 755 mmHg. It is released and rises to an altitude of 4.70 km, where the pressure is 499 mmHg and the temperature is -8.1°C. The volume of the balloon at this altitude is L.
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
The critical pressure, Pe, and the critical temperature, Te, of gas A are 3.040 × 10° Pa and 473 K, respectively. (i) Calculate the van der Waals constants, a and b, for this gas. (ii) Gas A obeys the van der Waals equation. Calculate the pressure exerted by one mole of gas A if the molar volume occupied by this gas is 2.75 L/mol at 298 K.
Which one or more of the following statements are true?(a) O2 will effuse faster than Cl2.(b) Effusion and diffusion are different names for the sameprocess.(c) Perfume molecules travel to your nose by the process ofeffusion.(d) The higher the density of a gas, the shorter the meanfree path.