Under similar conditions of pressure and temperature, 40 ml of slightly moist hydrogen chloride gas is mixed with 20 ml of ammonia gas,the final volume of gas at the same temperature and pressure will be

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Solution

$\begin{matrix} N H_{3 (g)} + & H C l_{g} \to & N H_{4} C l_{(s)} t = 0 & 20 m l & 40 m l & 0 t = t & 0 & 20 m l & s o l i d \end{matrix}$

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Under similar conditions of pressure and temperature, 40 ml of slightly moist hydrogen chloride gas is mixed with 20 ml of ammonia gas,the final volume of gas at the same temperature and pressure will be

40 m L

of slightly moist

H C l

gas is mixed with

20 m L

of ammonia gas, the final volume of gas at the same temperature and pressure will be :

400 m L

of ammonia gas at a pressure of

300 m m

and

200 m L

of hydrogen chloride gas at a pressure of

600 m m

are mixed in one litre evacuated flask. The pressure at normal temperature is :

Q. A certain mass of gas occupied a volume of 640 ml at a certain temperature and pressure. If the temperature is decreased by 40%, what will be the volume occupied by the same mass of gas under the same pressure?

Q. 400 mL of hydrogen gas at a pressure of 300 mm

H g

and 200 mL of hydrogen chloride gas at a pressure of 600 mm

H g

are mixed in a one litre evacuated flask. Calculate the resulting pressure (in

mm Hg

) of the mixture at the same temperature.

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Under similar conditions of pressure and temperature, 40 ml of slightly moist hydrogen chloride gas is mixed with 20 ml of ammonia gas,the final volume of gas at the same temperature and pressure will be

NH3(g)+HClg→NH4Cl(s)t=020ml40ml0t=t020mlsolid

$\begin{matrix} N H_{3 (g)} + & H C l_{g} \to & N H_{4} C l_{(s)} t = 0 & 20 m l & 40 m l & 0 t = t & 0 & 20 m l & s o l i d \end{matrix}$