Chemistry, asked by Anonymous, 10 months ago

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10 g of Hydrogen gas has a pressure of 0.95 × 10^5 N/m^2 at 27°C. If the volume remains constant and temprature is raised to 57°C. Find the pressure of the gas?

Answers

Answered by Anonymous

Solution :

Given :-

▪ Initial pressure of hydrogen = 95000 N/m $^2$

▪ Initial temperature of hydrogen = 27°C = 300K

▪ Final temperature of hydrogen = 57°C = 330K

To Find :-

▪ Final pressure of hydrogen.

Concept :-

This question is completely based on concept of 'Gay Lussac's law'.

As per Gay Lussac's law, At constant volume, pressure of a fixed amount of a gas varies directly with the temperature.

Mathematically,

$\bigstar\bf\pink{P\propto T}$

Calculation :-

$\implies\bf\:\dfrac{P_1}{T_1}=\dfrac{P_2}{T_2}\\ \\ \implies\sf\:\dfrac{95000}{300}=\dfrac{P_2}{330}\\ \\ \implies\sf\:P_2=\dfrac{95000\times 330}{300}\\ \\ \implies\underline{\boxed{\purple{\bf{P_2=1.045\times10^5\:Nm^{-2}}}}}$

Answered by XxpawanxX59

Explanation:

$<body bgcolor=red><marquee><font color=yellow>$ Reffer the attachment.

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10 g of Hydrogen gas has a pressure of 0.95 × 10^5 N/m^2 at 27°C. If the volume remains constant and temprature is raised to 57°C. Find the pressure of the gas?​