Question

750 ml of nitrogen gas is observed at 2.56atm. What is the pressure if the volume becomes 985ml?

Answer 1

Boyle's Law-

`\:\:\:\:\:\:\:\:\:\:\:\star\:\sf \underline{ P_1 \: V_1=P_2 \: V_2}\\`

(Pressure is inversely proportional to the volume)

Where-

• 
  `\sf V_1` = Initial volume
• 
  `\sf V_2` = Final volume
• 
  `\sf P_1` = Initial pressure
• 
  `\sf P_2` = Final pressure

As per question, we are given that -

• 
  `\sf V_1` = 750 mL
• 
  `\sf P_1` = 2.56 atm
• 
  `\sf V_2` = 985 mL

Now that we have all the required values and we are asked to find out the final pressure, so we can put the values and solve for the final pressure of nitrogen -

`\:\:\:\:\:\:\:\:\:\:\:\:\:\:\:\star\:\sf \underline{ P_1 \: V_1=P_2 \: V_2}`

`\:\:\:\: \:\:\:\:\:\:\longrightarrow \sf 2.56* 750 = P_2 * 985\\`

`\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf P_2 = (2.56 * 750)/(985)\\`

`\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf P_2 = \cancel{( 1920)/(985)}\\`

`\:\:\:\: \:\:\:\:\:\:\longrightarrow \sf P_2 = 1.94923........ \\`

`\:\:\:\:\:\:\:\:\:\:\longrightarrow \sf \underline{P_2 = 1.95 \: atm}\\`

Therefore,the pressure will become 1.95 atm if the volume becomes 985mL.