For an ideal gas, calculate the following quantities.(a) The pressure of the gas if 0.155 mol occupies 217 mL at 35°C.18.06atm(b) The temperature (in kelvins) at which 0.0290 mol occupies 1.00 L at 0.553 atm.235.9♥K(c) The number of moles in 4.50 L at -1°C and 745 torr. Remember 1atm = 760 torr.0.176x mol(d) The volume occupied by 8.72 x 10-3 mol at 30.°C and a pressure of 1.37 kPa. Remember 1 atm = 101.325 kPa1.60X L

The ideal gas law equation is:PV = nRTwhere:P is the pressure of the gas .V is the volume of the gas…

Answered: For an ideal gas, calculate the…

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...

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(a) A piston at 8.3 atm contains a gas that occupies a volume of 3.5 L. What pressure would have to be placed on the piston to force the volume to adjust to 1.36 L? ________atm(b) A piston at 51.0°C contains a gas that occupies a volume of 2.5 L. To what temperature would the gas have to be heated to increase the volume to 7 L at constant pressure? _______°C(c) A piston at 4695 torr contains a gas that occupies a volume of 4.7 L. What pressure would have to be placed on the piston to force the volume to adjust to 0.97 L? _______atm
At 105.1 oC and 0.4500 atm pressure, a gas occupies a volume of 0.600 L. How many liters will it occupy at 0.0 oC and 0.205 atm (760 torr = 1 atm = 101,325 Pa, R = 0.08206 L*atm/mol*K, K = 273.15 +C
A mixture containing 2.21 g each of CH4(g), C,H4(g) and CAH10(g) is contained in a 1.50 L flask at a temperature of 25°C. (a) Calculate the partial pressure of each of the gases in the mixture. PCH atm atm %3D PCH0 atm (b) Calculate the total pressure of the mixture. atm
What is the volume, in liters, occupied by a mixture of 15.2g Ne(g) and 34.8g Ar (g) at 7.24 bar pressure and 26.7C I QUESTION 2 A gas cylinder of 53.7 L volume contains N2(g) at a pressure of 28.2 atm and 26C. How many grams of Ne(g) must we add to this same cylinder to raise the total pressure to 75.0 atm? QUESTION 3 A 4.0 L sample of O2 gas has a pressure of 1.0 bar. A 2.0 L sample of N2 gas has a pressure of 2.0 bar. If these two samples are mixed and then compressed in a 2.0 L vessel, what is the final pressure of the mixture in atm? Assume that the temperature remains unchanged.
What is the volume, in liters, of 4.00 molesmoles of methane gas, CH4CH4, at 17 ∘C∘ and 2.00 atm? Express your answer with the appropriate units.
Calculate the number of moles of Cl2(g) (70.90 g/mol) in a volume of 352 mL at 27.5oC and a pressure of 0.953 atm. Your answer should have 3 sig figs.
.0380 of Mg strip reacted completly with 6 M HCL in the gas burret and 35.8 mL of hydrogen gas is collected over water at 20 c. The presure of the "wet" hydrogen gas is adjusted to the outside atmospheric pressure, a pressure of 747.50 torr. The vapor pressure of water at 20 c is 17.54 torr. Using the volume of hydrogen gas collected and the universal gas law, Pv=nRT, calculate the experimental number of moles of hydrogen produced.
What is the density, in g/L, of SF6 gas (146 amu) at 27°C and 0.500 atm pressure.
Three gases (CO, 02, and N) are trapped in individual bulbs of difterent volumes below. When the valves are opened, the individual gases expand and occupy the entire volume (10.00 L) of the apparatus. Assume that the temperature is constant. The mole fraction of each gas is equal to the partial pressure of a gas divided by the total pressure %3D What is the mole fraction of N2(g) in the mixture? (XN2 = PN2/Ptotal) Bulb Gas Volume (1) Pressure (atm) Carbon dioxide 3.00 1.00 Oxygen 1.00 1.00 Nitrogen 6.00 3.00 III O a 0.81 O b. 2.23 O 1.80 d. 0.500 0.654 f. The temperature must be known
A typical fluorescent light bulb contains argon gas and mercury vapor. (a) If the total gas pressure in a fluorescent light bulb is 307.4 Pa and the partial pressure of the argon gas is 306.1 Pa, what is the partial pressure of the mercury vapor? Pa(b) If a 930.-mL fluorescent bulb contains 4121 µg of argon gas and 81 µg of mercury vapor, what is the total gas pressure in the fluorescent bulb at 310. K? Pa
The pressure in atm, if 8.25 × 10 ^-2mole of an ideal gas occupies a volume of 255 ml at 115 deg C.
Assume that an exhaled breath of air consists of74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor.(a) If the total pressure of the gases is 0.985 atm, calculatethe partial pressure of each component of the mixture.(b) If the volume of the exhaled gas is 455 mL andits temperature is 37 °C, calculate the number of moles ofCO2 exhaled. (c) How many grams of glucose (C6H12O6)would need to be metabolized to produce this quantity ofCO2? (The chemical reaction is the same as that for combustionof C6H12O6. )

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