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Scrat [10]
3 years ago
13

A balloon contains 3.9 moles of helium at a pressure of 234 kPa and 67°C temperature. What is the balloon's volume in liters?

Chemistry
1 answer:
leonid [27]3 years ago
5 0

Answer:

47.1 L.

Explanation:

  • To solve these problems, we can use the general law of ideal gas: <em>PV = nRT.</em>

where, P is the pressure of the gas in atm (P = 234.0 kPa/101.325 ≅ 2.31 atm)  .

V is the volume of the gas in L (V = ??? L).

n is the no. of moles of the gas in mol (n = 3.9 mol).

R is the general gas constant (R = 0.082 L.atm/mol.K),

T is the temperature of the gas in K (T = 67.0 °C + 273.15 = 340.15 K).

The volume of the gas = nRT/P.

<em>∴ V = nRT/P </em>= (3.9 mol)(0.082 L.atm/mol.K)(340.15 K)/(2.31 atm) = <em>47.1 L.</em>

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First, look at what you have and look at the equations you can use to solve this problem. The best equation would be PV=nRT.

P being pressure, V being volume, n being moles, R being the gas constant, and T being temperature.

Before you start doing any of the math, make sure of two things. Since you're looking for pressure, you'll need a gas constant. When I did the problem, I used the gas constant of atm or atmospheres which is .0821.

Also! Remember to always convert celsius into kelvin, to do this, add 273 to the given celsius degree. After this is all set and done, your equation should look like this:

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Multiply everything on the top and divide by the bottom and you should receive the final answer of .774atm.

Hope this helps!

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