What size tank would be needed to contain this same amount of hel...

Question

What size tank would be needed to contain this same amount of helium at atmospheric pressure (1 atm)?

Accepted Answer

Hey everyone for this problem we have a sample of nitrogen gas and we're being asked if the pressure is increased, what volume would nitrogen occupy. So we're dealing with volume temperature and pressure here. So let's go ahead and write out our ideal gas law which is P. V. Equals N. R. T. And for this problem we are given to pressures and two volumes. They don't tell us anything about our sample of nitrogen increasing in terms of um moles or mass. So we can go ahead and cancel that out because here it's constant. Are gas constant R. Is also constant so we can cross that out and our temperature, they tell us what the temperature is but our temperature is not changing so it's also constant and we'll cross that out. So what we're left with is just pressure and volume. And because they give us to and they're changing, we can rewrite this equation two Bp one Times V one is equal to P two times v. two and we'll go ahead and plug in what we know based off what was given. So our first pressure Is 723 tour And the volume that goes with that pressure is 0.55 No leaders. And this is equal to r. p. two Which is 925 tour Times V. Two. Which is what we're solving for. We want to know what a volume would nitrogen occupy. So let's go ahead and solve for v. two. When we do the left side of our equation, we get 2,027,871 is equal to 925 times. V two. We'll divide both sides by And we're left with V two is equal to 30 .1 Mil leaders. And that is the end of this problem, and that is answer choice. C. I hope this was helpful.

What size tank would be needed to contain this same amount of helium at atmospheric pressure (1 atm)?

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