The density of a gas is 1.43 g/l at a temperature of 23 ∘c and a pressure of 0.789 atm. calculate the molar mass of the gas.

44.04 g/mol

Explanation:

Ideal gas law in terms of density:

where,

P = pressure of the gas  = 0.789 atm

V = volume of the gas

T = temperature of the gas  =

n = number of moles of the gas

R = gas constant = 0.0821 Latm/moleK

M = molar mass of gas

w = mass of gas

= density =1.43 g/ml

Thus molar mass of the gas is 44.04 g/mol

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :