A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is atm.

Partial pressure of Ne is 0.61 atm.

Explanation:

Mole fraction of a gas in mixture = (no. of moles of the gas in mixture)/(total no. of moles of gases in mixture)

Here, total no. of moles of gases = (0.32 + 0.56) moles = 0.88 moles

So, mole fraction of Ne in mixture,

Let's assume both He and Ne along with their mixture behaves ideally,

Hence, in accordance with Dalton's law of partial pressure-

Where, and are partial pressure of Ne and total pressure respectively.

So,  

So, partial pressure of Ne is 0.61 atm.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: