Use the van der Waals equation of state to calculate the pressure of 2.60 mol of Cl2 at 469 K in a 5.60 L vessel. Use this list of van der Waals constants. CH4 2.303 2.273  0.0431  CO2 3.658 3.610  0.0429  Cl2 6.343 6.260  0.0542  NH3 4.225 4.170  0.0371  H2O 5.537 5.465  0.0305  Xe 4.192 4.137  0.0516 I've tried a few different ways and I'm still getting it wrong.

The combustion of propane is described by the chemical equation C3H8 (g) +502(g) → 3CO2(g) + 4H₂O(g) . If we have a partial pressure of 0.375 bar of propane as the reactant, what partial pressure of oxygen will we need to have a perfect amount to consume all of the propane with no unreacted propane or oxygen left over at the end of the reaction? 1.13 kPa 0.0750 bar 0.375 bar 1.88 bar

Real gases can exist under conditions other than STP. True O False

Please do not round off sig figs in calculations until final answer. Thank you.

What are the units of a? What are the units of b? For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. atm Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 55.0 °C with a molar volume of 0.515 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm Explanation Check

A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 72 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 27 s for 1.0 L of 02 gas to effuse. 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.) 367.1175859 X g/mol

A sample of unknown gas weighs 2.80 g and occupies 710 mL at 740 mmHg and 70 ∘C. What is the molar mass of the unknown gas?

A 3.0L sample of gas at 1.0 atm and 0.0℃ is heated to 85℃. Calculate the final volume. The pressure remains constant.

Match the characteristic of gases described below to the postulates of the kinetic molecular theory that best explain that characteristic. (Note: You may need to list more than one postulate.) The pressure of a gas in a fixed volume increases when its temperature increases. Select one or more: The average kinetic energies of gas particles increase with an increase in temperature. Gas particles are widely spaced. A gas consists of many small particles in rapid, random motion. The total volume of the molecules themselves is very small compared to the volume of the container. There are virtually no attractive forces between gas particles.

A 2.15 g2.15 g sample of an unknown gas at 59 ∘C59⁢ ∘C and 1.00 atm1.00 atm is stored in a 1.95 L1.95 L flask. What is the density of the gas?   What is the molar mass of the gas?