A gas has a Henry's law constant of 0.112 M>atm. What total volume of solution is needed to completely dissolve 1.65 L of the gas at a pressure of 725 torr and a temperature of 25 °C?

Video transcript

I have one. So we have 815 tour In 24.5°C. You ask, calculate the amount of solution in leaders Regard to dissolve 6.72 L of gas with Henry's law constant of 0.129 polarity per atmosphere. We call that Henry's law society, ability of gas, similarity, people to Henry's law constant, similarity per atmosphere. That was the partial pressure of a gas. We know that polarity. It was malls lot about. Leaders of the solution. We need to first find the moles. We're gonna use the ideal gas law which is gonna be P. P. He goes, N. R. T. We're gonna rearrange this is all for N. Get PB about R. T. We're looking for N. MP. S. and 15 Tour. And we have 760 tour and one atmosphere. Give us 1.0724 atmosphere. The volume is 6.72 L. R 0.08206. Later sounds atmosphere. What about moles? How's kelvin? And for the temperature 24.5°C, we need to add 273.15 To get into Kelvin. Gonna get 297.65 Kelvin. So now if you play this into the equation, I'm gonna get in, it goes 1.07 2 4 atmosphere. That was 6.72 l Divided by 0.0806. Later times atmosphere about Moles and Kelvin From 297.65 Kelvin. It was 0.29 five moles. Then I we can rearrange Henry's law. To solve for leaders, We're gonna have a solid body of a gas equal to Henry's law constant. The partial pressure of the gas. We're gonna have moles of gas here. What about leaders of the solution? Your hands are constant. Find the pressure of a gas. We're gonna get leaders of the solution equal to malls of gas. I thought about him was like constant. The partial pressure of the gas. I'm gonna get 0.2950 malls five x 0.12 non polarity or atmosphere 1.0724. Atmosphere for the leader of the solution, We get 2.13 L. Thanks for watching my video and I hope it was helpful.