EXAM PRACTICE

The STP (standard temperature and pressure) condition stands for:

A balloon filled with an ideal gas is taken from the surface of the sea to a depth of $100$ m. What will be its volume in terms of its original volume?  

Calculate the temperature of $4.0$moles of a gas occupying $5 {\mathrm{dm}}^3$ at $3.32$bar. (Take, $\mathrm{R} = 0.083 \mathrm{bar} {\mathrm{dm}}^3 {\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$). 

Determine the pressure of a gas, when its volume is $250 \mathrm{mL}$ initially, the gas is expanded to volume of $1000 \mathrm{mL}$ and the pressure of $0.4$ atmosphere. Assume that temperature during the reaction remains constant. 

The volume occupied by a given gas was $5.6 {\mathrm{dm}}^3$ when the pressure was $2$ atmosphere. If the pressure is increased by $20\%$, calculate the new volume of the gas. 

A gas is enclosed in a vessel at standard temperature. Find out the temperature at which the volume of enclosed gas will be $1/6$ of its initial volume. (Given that the pressure remain constant) 

$6 {\mathrm{dm}}^3$ of dry gas is present at temperature of $27°\mathrm{C}$ and pressure of $700$ mm of Hg. Determine the volume of gas at STP 

 Moist nitrogen at a pressure of $700 \mathrm{mm}$ of Hg and temperature of $300 \mathrm{K}$ is found to occupy a volume of $100 {\mathrm{cm}}^3$. Determine the volume of dry nitrogen gas at STP. (Take, aqueous tension at $27°\mathrm{C}$ is $15 \mathrm{mm}$ of Hg)