Problem: Hydrogen and oxygen gas are mixed in a 7.75 L flask at 65°C and contains 0.482 g of hydrogen and 4.98 g of oxygen. What is the partial pressure of oxygen in the flask?a. 33.5 atmb. 0.557 atmc. 67 atmd. 1.11 atme. 0.043 atm

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FREE Expert Solution

We’re being asked to calculate the partial pressure of oxygen in a 7.75 L flask at 65°C.

We will use ideal gas equation to calculate for the pressure:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K

But first, we have to calculate the amount of oxygen (O2) in moles.

Problem Details

Hydrogen and oxygen gas are mixed in a 7.75 L flask at 65°C and contains 0.482 g of hydrogen and 4.98 g of oxygen. What is the partial pressure of oxygen in the flask?

a. 33.5 atm

b. 0.557 atm

c. 67 atm

d. 1.11 atm

e. 0.043 atm

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofHydrogen and oxygen gas are mixed in a 7.75 L flask at 65°C ...as medium difficulty.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ratliff's class at USF.