Hey sample of helium occupies 235 ml at 788 tour and 25°c. if the sample is condensed into a 0.115 l flask what will be the new pressure assuming constant temperature?

The new pressure of helium gas assuming constant temperature is equal to 1610.26 Torr.

Given the following data:

Conversion:

Initial volume = 235 mL to L =

To determine the new pressure assuming constant temperature, we would apply Boyle's law:

Mathematically, Boyle's law is given by the formula;

Where;

Substituting the given parameters into the formula, we have;

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the system is in constant temperature

so it follows Boyle's law

i.e.P1V1=P2P2

where P1=initial pressure=788 tour

P2=final pressure= ?

V1=initial volume=235 ml

V2=final volume=0.115 ml

16

explanation:

the marks go by 4s

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o