The partial stress of H2 is 737.47 mmHg Let's observe the Ideal Gas Law to find out the whole mols.
We count on that the closed vessel has 1L of volume
- P.V=n.R.T
- We must convert mmHg to atm. 760 mmHg.
- 1 atm
- 755 mmHg (755/760) = 0.993 atm
- 0.993 m.1L=n.0.082 L.atm/mol.K .
- 293 K(0.993 atm 1.1L)/(0.082mol.K /L.atm).
- 293K = n
- 0.0413mols = n
These are the whole moles. Now we are able to know the moles of water vapor, to discover the molar fraction of it.
- P.V=n.R.T
- 760 mmHg. 1 atm
- 17.5 mmHg (17.5 mmHg / 760 mmHg)=0.0230 atm
- 0.0230 m.1L=n.0.082 L.atm/mol.K.293 K(0.0230atm.1L)/(0.082mol.K/L.atm .293K)=n 9.58 × 10 ^ 4 mols = n.
- Molar fraction = mols )f gas/general mols.
- Molar fraction water vapor =9.58×10^ -four mols / 0.0413 mols
- Sum of molar fraction =1
- 1 - 9.58 × 10 ^ 4 × mols / 0.0413 ×mols = molar fraction H2
- 0.9767 = molar fraction H2
- H2 pressure / Total pressure =molar fraction H2
- H2 pressure / 55mmHg = =0.9767 0.9767 = h2 pressure =755 mmHg.
- 737,47 mmHg.
<h3>What is a mole fraction?</h3>
Mole fraction is a unit of concentration, described to be identical to the variety of moles of an issue divided through the whole variety of moles of a solution. Because it's miles a ratio, mole fraction is a unitless expression.
Thus it is clear that the partial pressure of H2 is 737,47 mmHg.
To learn more about partial pressure refer to the link :
brainly.com/question/19813237
<h3 />
Typically the solvent used for the chromatography is rather volatile. So, its likely that the entire solvent will evaporate prior to the completion of the chromatography if the container isn't covered.
Answer:
The air pressure on the inner side of the can balances that on the outside of the can.
Explanation:
Indeed the air pressure might crush a properly-sealed air-tight can during the descent. The reason is that the air pressure on the outside of the can exceeds that on the inside. The force that pushes the wall inwards exceeds the force that pushes the wall outwards. It's the pressure difference that crushes the can. However, that's not exactly the case for the "empty soft-drink can" here.
The question states that the can is already "empty." Therefore, it is quite reasonable to assume that the can was already opened. In other words, the can would no longer be air-tight. Air particles could freely enter and leave the can. As a result, when the can is brought down a mountain, air enters the can. As long as the can stays open, there would be enough air particles on the inside to balances the pressure. A pressure difference will not build up. That ensures that the can stays intact.
Answer:
The Answer is A, The iron-nickel alloy melts due to hot temperatures.
Explanation:
I took the test on edgenuity :) hope this helps.
