An 18.0 L container holds 16.0 g of oxygen gas (O2) at 45.0 °C. (a) Look up the molar mass of oxygen gas, and use that to determine the amount of gas. (b) Use the ideal gas law to find the pressure in the container.
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An 18.0 L container holds 16.0 g of oxygen gas (O2) at 45.0 °C.
(a) Look up the molar mass of oxygen gas, and use that to determine the amount
of gas.
(b) Use the ideal
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- A glass container encloses a low pressure of 02 gas at 298 K. The molecular weight of 02 is 32.0 g/mol. (A) Calculate the mean squared velocity, v², of these molecules in units of m²/s². (B) Find the root mean squared speed along the x-axis, Vx. (C) Would Vx be lower, higher, or the same under the same conditions if the gas were He instead of 02? Please explain your answer in 15 words or less.(a) An ideal gas occupies a volume of 1.2 cm³ at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container. molecules (b) If the pressure of the 1.2-cm³ volume is reduced to 2.2 x 10-11 Pa (an extremely good vacuum) while the temperature remains constant, how many moles of gas remain in the container? molIf 2.00 mol of nitrogen gas (N2) are placed in a cubic box, 34.0 cm on each side, at 2.50 atm of pressure, what is the rms speed of the nitrogen molecules? 730.13 * m/s
- An ideal monatomic gas is contained in a vessel of constant volume 0.220 m3. The initial temperature and pressure of the gas are 300 K and 5.00 atm, respectively. The goal of this problem is to find the temperature and pressure of the gas after 29.0 kJ of thermal energy is supplied to the gas. (a) Use the ideal gas law and initial conditions to calculate the number of moles of gas in the vessel. mol (b) Find the specific heat of the gas. /K (c) What is the work done by the gas during this process? kJ (d) Use the first law of thermodynamics to find the change in internal energy of the gas. kJ (e) Find the change in temperature of the gas. K (f) Calculate the final temperature of the gas. K (g) Use the ideal gas expression to find the final pressure of the gas.One cylinder contains helium gas and another contains krypton gas at the same temperature. Mark each of these statements true, false, or impossible to determine from the given information. (a) The rms speeds of atoms in thetwo gases are the same. (b) The average kinetic energies of atoms in the two gases are the same. (c) The internal energies of 1 mole of gas in each cylinder are the same. (d) The pressures in the two cylinders are the same.(a) What is the gauge pressure in a 25.0oC car tire containing 3.60 mol of gas in a 30.0 L volume? (b) What will its gauge pressure be if you add 1.00 L of gas originally at atmospheric pressure and 25.0oC? Assume the temperature returns to 25.0oC and the volume remains constant.