Question

If have a volume of 18 L of a gas at a temperature of 272 K and a pressure of 90 atm, what will be the pressure of the gas if raise the temperature to 274 Kand decrease the volume to 12 L?

Answer 1

P₂ ≅ 100 atm (1 sig. fig. based on the given value of P₁ = 90 atm)

Step-by-step explanation:

Given:

P₁ = 90 atm P₂ = ?

V₁ = 18 Liters(L) L₂ = 12 Liters(L)

=> decrease volume => increase pressure

=> volume ratio that will increase 90 atm is (18L/12L)

T₁ = 272 Kelvin(K) T₂ = 274 Kelvin(K)

=> increase temperature => increase pressure

=> temperature ratio that will increase 90 atm is (274K/272K)

n₁ = moles = constant n₂ = n₁ = constant

P₂ = 90 atm x (18L/12L) x (274K/272K) = 135.9926471 atm (calculator)

By rule of sig. figs., the final answer should be rounded to an accuracy equal to the 'measured' data value having the least number of sig. figs. This means P₂ ≅ 100 atm based on the given value of P₁ = 90 atm.