Question

A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 liters, what must the new pressure be?

Answer 1

Answer of this question is 0.5atm

___________________________

Given :-

• Initial volume of gas = 4L
• Initial pressure of gas = 2atm
• Final volume of gas = 16L

To Find :-

• Final pressure of gas

Solution :-

▪ As per boyle's law, change in pressure of gas at constant temperature is inversely proportional to the chane in volume of gas.

$\rightarrow\bf\:P_1V_1=P_2V_2\\ \\ \rightarrow\sf\:2\times 4= P_2\times 16\\ \\ \rightarrow\sf\:P_2=\dfrac{8}{16}\\ \\ \rightarrow\underline{\underline{\large{\bf{P_2=0.5\:atm}}}}$

Answer 2

Answer:

Concept :

Boyle's law is a connection that defines how a gas compressed and expands at a fixed temperature. It is also referred as Mariotte's law. This empirical relationship, proposed by scientist Robert Boyle in 1662, asserts that at constant temperature, A given quantity of gas's pressure (p) decreases inversely with its volume (v), resulting in pv = k, a constant.

Given :

The pressure of a gas with a volume of 4 litres is 2 atm. What is the new pressure if the volume is increased to 16 litres?

Find :

To find the new pressure.

Answer :

the new pressure is 0.5

Explanation :

Given

$V1 = 4 ltr\\V2 = 16 ltr\\P1 = 2 atm\\P2 = ?$

to find the pressure we use Boyle's law

$P1V1 = P2V2 (Boyles law)\\2*4=P2*16\\8 = P2*16\\8/16 = P2\\P2 = 1/2\\P2 = 0.5$

the new pressure is 0.5

Under the assumption of an ideal gas, the law can be inferred from the kinetic theory of gases. Real gases satisfy Boyle's law at suitably low pressures, while the product pv tends to decrease slightly at increasing pressures. When the gas begins to stray from its optimal behaviour, it reaches certain pressures.

#SPJ2