An experiment shows that a 115 mLmL gas sample has a mass of 0.169 gg at a pressure of 700 mmHgmmHg and a temperature of 30 ∘C∘C. What is the molar mass of the gas?

39.7g/mol

Explanation:

To calculate the molar mass of the gas, first let us calculate the number of mole of the gas. This is illustrated below:

Data obtained from the question include:

V = 115mL = 0.115L

P = 700mmHg

Recall: 760mmHg = 1atm

700mmHg = 700/760 = 0.92atm

T = 30°C = 30 +273 = 303K

R = 0.082atm.L/Kmol

n =?

PV = nRT

n = PV/RT

n = (0.92 x 0.115)/(0.082x303)

n = 4.26x10^-3mol

Now we can obtain the molar mass of the gas as follows:

Mass of the gas = 0.169g

Number of mole of the gas = 4.26x10^-3mol

Molar Mass of gas =?

Number of mole = Mass /Molar Mass

Molar Mass = Mass/number of mole

Molar Mass of the gas = 0.169/4.26x10^-3

Molar Mass of the gas = 39.7g/mol

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.