Amixture of 10.0 g of ne and 10.0 g ar have a total pressure of 1.6 atm. what is the partial pressure of ne?

1.1atm

Explanation: A mixture of 10.0 g of Ne and 10.0 g of Ar has a total pressure of 1.6 atm. What is the partial pressure of Ne?

a. 1.1 atm

b. 0.8 atm

c. 0.54 atm

d. 0.40 atm

e. 1.3 atm

In any mixture of gases, the partial pressure of the individual components of the mixture is the pressure which that component would normally occupy if it were present alone under the same circumstance. To calculate the partial pressure (p) of Ne in a mixture of Ne and Ar, the partial pressure of a gas in a mixture is given by mole fraction (X) of the gas multiplied by the total pressure (P) of the mixture.

n Ne = 10g /20.18 g/gmol = 0.4955 moles

n Ar = 10g /39.95 g/gmol = 0.2503 moles

Total number of moles = 0.4955 + 0.2503 = 0.7458 moles

X Ne = 0.4955 / 0.7458 = 0.6644

p Ne = (X Ne)(P)

= 0.6644 x 1.6 = 1.063 atm

Which is approximately 1.1atm as answer

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.

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