How many moles of gas are required to exert 15.4 atm of pressure in a 2.92 L container at 32.0°C

1.8 moles

Explanation:

Number of moles = ?

Pressure = 15.4 atm

Volume = 2.92L

Temperature = 32°C = (32 + 273.15)K = 305.15K

From ideal gas equation,

PV = nRT

P = pressure of the ideal gas

V = volume in which the gas occupies

n = number of moles

R = ideal gas constant = 0.082J/mol.K

T = temperature of the gas

PV = nRT

n = PV / RT

n = (15.4 * 2.92) / (0.082 * 305.15)

n = (44.968 / 25.0223)

n = 1.797 moles = 1.8 moles

Number of moles of the gas is 1.8 moles

a) the particles of the chair are strongly held together.

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.