What will be the minimum pressure required to compress $500 d m^{3}$ of air at $1 b a r$ to $200 d m^{3}$ at $30^{\circ} C$ ?

Open in App

Solution

According to ideal gas equation, $P_{1} V_{1} = P_{2} V_{2}$

Here $P_{1} = 1 b a r, V_{1} = 500 d m^{3}, V_{2} = 200 d m^{3}$

Then $P_{2} = \frac{1 \times 500}{200} = 2.5 b a r$

Suggest Corrections

Similar questions

What will be the minimum pressure required to compress 500 dm³ of air at 1 bar to 200 dm³ at 30°C?

What will be the minimum pressure required to compress 500 $d m^{3}$ of air at 1 bar to 200 $d m^{3}$ at $30^{0} C$ ?

^{3}

^{3}

^{0}

Join BYJU'S Learning Program