NEED HELP ASAP; PLEASE SHOW YOUR WORK.
The volume of a sample of chlorine gas is 8.00 liters at 45.0 degrees Celsius and 0.966 atm. How many moles of chlorine are present in the sample? R = 0.0821 (atm)(L)(mol-1)(K-1)

n = 0.3 mol

Explanation:

Given data:

Volume of gas = 8.0 L

Temperature of gas = 45 °C (45+273 = 318 K)

Pressure of gas = 0.966 atm

Moles of gas present = ?

Ideal gas constant = R = 0.021 atm.L/mol.K

Solution:

Formula:

PV = nRT

P = Pressure

V = volume

n = number of moles

R = ideal gas constant

T = temperature

Now we will put the values:

0.966 atm × 8 L = n × 0.0821 atm.L/mol.K × 318 K

7.728 atm.L = n × 26.12  atm.L/mol

7.728 atm.L / 26.12  atm.L/mol = n

n = 0.3 mol

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.

you need to have a picture of the atom that way we can answer it