Answered

Boyle's Law expresses the pressure-volume
relationship as P.V1 = P2V2, so you will need to solve this equation for the unknown quantity and then plug in your known values to calculate the unknown.
What pressure would it take to compress 350. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature?​

Answer :

znk

Answer:

[tex]\large \boxed{\text{175. atm}}[/tex]

Explanation:

Data:

p₁ = 1.00 atm; V₁ = 350.      L

p₂ = ?;             V₂ =     2.00 L

Calculation:

[tex]\begin{array}{rcl}p_{1}V_{1} & = & p_{2}V_{2}\\\text{1.00 atm} \times \text{350. L} & = & p_{2} \times\text{2.00 L}\\\text{350. atm} & = & 2.00p_{2}\\p_{2} & = & \dfrac{\text{350. atm}}{2.00}\\\\& = &\textbf{175. atm}\\\end{array}\\\text{It would take a pressure of $\large \boxed{\textbf{175. atm}}$ to compress the gas.}[/tex]

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