Asample of an ideal gas has a mass of 0.311 grams. its volume is 0.225 l at a temperature of 55oc and a pressure of 1.166 atm. find its molar mass.

The molar mass of the gas is 31.9 g/mol

Explanation:

Step 1: Data given

Mass of the gas = 0.311 grams

Volume = 0.225 L

Temperature = 55.0 °C

Pressure = 1.166 atm

Step 2: Calculate moles

p*V = n*R*T

⇒ p = the pressure of the gas = 1.166 atm

⇒ V = the volume of the gas = 0.225L

⇒ n= the number of moles of gas = TO BE DETERMINED

⇒ R = the ideal gas constant = 0.08206 L*atm/K*mol

⇒ T = the temperature = 55.0 °C = 328 Kelvin

n = (p*V)/(R*T)

n = (1.166*0.225)/(0.08206*328)

n = 0.009747

Step 3: Calculate the molar mass

Molar mass = mass / moles

Molar mass = 0.311 grams / 0.009747

Molar mass = 31.9 g/mol

The molar mass of the gas is 31.9 g/mol

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of carbon is as shown here in the image.

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g