In a victor Mayer's experiment 0.33g of organic liquid of molecular weight 120g/mol was vaporized at 293k and 1.013 *10 N/ m calculate the vol in cm3 of air displaced

66.13 cm³

Explanation:

Using the ideal gas equation, PV = mRT/M where P = pressure = 1.013 × 10⁵ N/m², V = volume of liquid vaporized = volume of air displaced, m = mass of organic liquid = 0.33 g, M = molar mass of gas = 120 g/mol and R = molar gas constant = 8.314 J/mol-K and T = temperature at vaporization = 293 K.

PV = mRT/M

So, V = mRT/PM

Substituting the values of the variables into the equation, we have

V = 0.33 g × 8.314 J/mol-K × 293 K/(1.013 × 10⁵ N/m² × 120 g/mol)

V = 803.881/121.56 × 10⁻⁵ m³

V = 6.613 × 10⁻⁵ m³

V = 6.613 × 10⁻⁵ × 1m³

V = 6.613 × 10⁻⁵ × 10⁶ cm³

V = 6.613 × 10 cm³

V = 66.13 cm³

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots

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