A sample of phosgene gas (COCl2) is kept at 850 torr and 35.0 °C. Determine its density.

A 25.0-L reaction vessel containing a mixture of CO₂ and excess F₂ is set up at 125 °C and 3.50 atm of pressure. According to the equation CO₂(g) + 4 F₂(g) → CF₄(g) + 2 OF₂(g), a spark ignites CO₂, resulting in its complete combustion. The temperature returns to 125 °C after the reaction, and the pressure of the mixture of product gases (CF₄, OF₂, and unreacted F₂) is found to be 2.85 atm. What are the partial pressures of the individual gases in the product mixture?

A mixture of Ba(BrO₃)₂ and Ba(BrO₂)₂ weighing 8.00 g was placed in a 5.00 L reaction vessel. The vessel was then heated to 800°C and both compounds decomposed forming BaBr₂(s) and O₂(g). If the vessel has a final pressure of 0.8968 atm, calculate the mass of each compound before decomposition.

H₂SO₃ decomposes into liquid water and SO₂ gas. Calculate the volume of SO₂ gas that would be produced at 1 atm and 300 °F from 5.60 g of H₂SO₃

At 15.0°C, a gas occupies a volume of 35.0 L and has a pressure of 136 atm. Calculate the volume (in L) it occupies at STP.

A newly discovered planet has a surface temperature of about 970 K and a pressure of 65 Earth atmospheres. These conditions define "STP" on this planet. Calculate the standard molar volume (in L) of gas on this planet.

Calculate the molar mass of a gas if its density at STP is 1.827 g/L.

Identify which of the following statements are false. 

i) The molecules from food responsible for its smell travel to your nose by the process of diffusion. 

ii)  F₂ will effuse faster than Kr.

iii) The higher the molar mass, the higher the effusion rate. 

iv) Effusion and diffusion are different processes.

v) Heavier molecules take more time to effuse. 

Arrange in order of increasing rate of effusion: Cl₂, Ar, HI.

How fast would ammonia (NH₃) molecules effuse compared to carbon dioxide (CO₂) molecules? Determine the ratio of rates of effusion and answer using three significant figures.

Calculate the temperature wherein SO₂ molecules will have the same mean speed as NO₂ molecules at 63.0°C. Report the answer in degrees celsius.  

Identify the gas that would have a lower mean speed: Kr at 15.0°C or Cl₂ at 300 K.

At 298 K, calculate the root mean square velocity and kinetic energy of CO, CO₂, and SeO₃. Which gas has the greatest velocity? The greatest kinetic energy? The greatest effusion rate?