Consider equimolar samples of different ideal gases at the same volume and temperature. Gas A has a higher molar mass than gas B.   Compare the pressures. A>B A=B AB A=B AB A=B A

Three identical balloons (shown below) are filled to the same volume. Temperature and pressure are kept constant (25°C and 101.3 kPa, respectively). Which balloon contains the smallest mass of gas? Explain your reasoning.

A bottle of N2O3(G) has a pressure of 0.475 atm. When the absolute temperature of the N2O3 (G) is tripled, the gas completly decomposes, producing NO2 (g) and NO(G). Calculate the final pressure of the gas mixture, assuming that the bottle volume does not change. Answer should be in atm.

Constants | Periodic Table A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure conditions. It required 105 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 29 s for 1.0 L of O2 gas to effuse. ▾ Part A Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) Express your answer in grams per mol to two significant figures. M = Ο ΑΣΦ Submit Request Answer 3+ < Return to Assignment Provide Feedback a % ? g/mol MacBook Pro 曲 C

Container A holds 1600 mL of ideal gas at 3.8 atm, 21 °C. Container B holds 400 mL of ideal gas at 6.9 atm, 50 °C. If the gases are allowed to mix together, and the final temperature is 35 °C, what is the pressure (in atm) of the mixed gas? R = 0.0821 (L atm/K mol). Keep two digits after decimal.

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A particular gas has an initial volume of 5.29 L and an initial temperature of 213.3 K. If the volume changes to 38.2 L, calculate the new temperature in K.

A cylinder is filled with 10.0L of gas and a piston is put into it. The initial pressure of the gas is measured to be 109. kPa. The piston is now pulled up, expanding the gas, until the gas has a final volume of 63.0L. Calculate the final pressure of the gas. Round your answer to 3 significant digits.

A 1.25 g sample of an unknown gas at 47 ∘C and 1.00 atm is stored in a 2.55 L flask. What is the density of the gas? density:   g/L   What is the molar mass of the gas? molar mass:   g/mol

[References] An ideal gas is contained in a cylinder with a volume of 4.2 x 10° mL at a temperature of 30.°C and a pressure of 700. torr. The gas is then compresse 23 mL, and the temperature is raised to 800.°C. What is the new pressure of the gas? Pressure torr