Gases questions | form five Chemistry

Using kinetic theory of gases, state four properties of an ideal gas.

a sample of ammonia gas with a volume of 3.5dm³ at a pressure of 1.68atm was compressed to a volume of 1.35dm³ at constant temperature.

1. Calculate the final pressure of the gas.
2. Name and state the governing gas law in (i)

Define the following:

1. Relative density of a gas.
2. Normal density of a gas.

1. Show that the relative molecular mass of ethanoic vapor at 1 atm pressure and 400K gave a result of 2.74g/dm³. Assuming ideal condition, calculate the apparent molecular weight of ethanoic acid under these conditions.
2. What can you deduce from your results in (i)? Briefly explain.

A 0.0721g of water vaporised at 150^oC and 755 mmHg pressure occupied a volume of 140cm³. Show that the relative molecular mass of water vapour proves the formula for steam.

State why was it necessary to modify the ideal gas equation and show how the modified equation looks like. Define all symbols in the equation.

Briefly explain why beyond certain temperatures gases cannot be liquefied.

One mole of diethyl ether occupies 1.5 litres at 227^oC. Calculate the pressure if the Van der Waals constants for diethyl ether are : a=17.38 atm.litre²mol^-1 and b=0.134 litre mol^-1.

Define the following terms with reference to gases:

1. Critical temperature
2. Critical volume
3. Critical pressure

From the ideal gas equation , derive the relationship between density of a gas in grams per dm³, the gas pressure in atmosphere , the temperature (T) in kelvin, the relative molecular mass of a gas (Mr) and the gas constant , R.