Standard or Normal Temperature and Pressure (STP or NTP)

A gas is allowed to expand at a constant temperature from an initial volume of $300 \mathrm{ml}$ to a final volume of $1800 \mathrm{ml}$. At the end of the expansion the pressure of the gas was found to be $1 \mathrm{atm}$. What was the initial pressure of the gas?

The pressure on one mole of a gas at STP is doubled and the temperature is raised to $546 \mathrm{K}$. What is the final volume of the gas? (one mole of a gas occupies a volume of $22.4$ litres at STP). Temperature in Kelvin is $273.15$.

Define STP or NTP. What are its values? Why is it necessary to compare gases at STP?

What is the boiling point of water on the Kelvin scale?

What is the need for the Kelvin scale of temperature?

What is absolute scale of temperature? Write the value of Kelvin zero in centigrade. What is 'absolute zero'?

A certain volume of a gas is kept at ${77}^{\mathrm{o}}\mathrm{C}$. When the temperature is decreased by ${20}^{\mathrm{o}}\mathrm{C}$ the gas occupies a volume of $900 \mathrm{ml}$. What was the initial volume of the gas (pressure constant)?

$60 {\mathrm{cm}}^3$ of oxygen was added to $24 {\mathrm{cm}}^3$ of carbon monoxide, and the mixture was ignited. Calculate the volume of carbon dioxide formed.

$60 {\mathrm{cm}}^3$ of oxygen was added to $24 {\mathrm{cm}}^3$ of carbon monoxide, and the mixture was ignited. Calculate the volume of oxygen used up.

The molecular theory accounts for the pressure exerted by a gas in a closed vessel as a result of the gas molecules striking against the walls of the vessel.

How will the pressure change if the volume is halved, keeping the temperature constant?

The molecular theory accounts for the pressure exerted by a gas in a closed vessel as a result of the gas molecules striking against the walls of the vessel.

How will the pressure change if the temperature is doubled keeping the volume constant?

A fixed mass of gas has a volume of $750 \mathrm{c}.\mathrm{c}.$ at $-{23}^{\mathrm{o}}\mathrm{C}$ and $800 \mathrm{mm}$ pressure. Calculate the pressure for which the volume will be $720 \mathrm{c}.\mathrm{c}.$ the temperature being $-3^{\mathrm{o}}\mathrm{C}$.

From the equation, ${\mathrm{N}}_2+3{\mathrm{H}}_2=2{\mathrm{NH}}_3$, calculate the volume of ammonia gas formed when $6$ litres of hydrogen react with excess nitrogen, all volume being measured at STP.

State Charles’ Law. Give its mathematical representation and graphical representation.

State Boyle's Law. Give its mathematical representation and graphical representation.

Explain 'Kinetic Molecular Theory'.