Chemistry: The empirical formula of a compound is ch. at 200 degrees celsius, 0.242 of this compound occupies 97.2ml at a pressure of 0.740atm. what is the molecular formula of the compound ?

The pressure of that gas will decrease.....

The empirical formula of a compound is ch. at 200

Ответ:

lbelle

07.01.2022

Chemistry

C₁₀H₁₀

Explanation:

We can use the Ideal Gas Law to solve this problem:

pV = nRT

Since n = m/M, the equation becomes

pV = (m/M)RT

Data:

p = 0.740 atm

V = 92.7 mL

m = 0.212 g

R = 0.082 16 L·atm·K⁻¹mol⁻¹

T =200 °C

Calculations:

(a) Convert the volume to litres

V = 92.7 mL = 0.0927 L

(b) Convert the temperature to kelvins

T = (200 + 273.15) = 473.15 K

$\begin{array}{rcl}\\pV&=&\dfrac{m}{M}RT\\\\\text{0.740 atm} \times \text{0.0972 L} & = &\dfrac{\text{0.242 g}}{M} \times 0.08206 \text{L}\cdot\text{atm}\cdot\text{K}^{-1}\text{mol}^{-1} \times \text{473.15 K}\\\\0.07193 & = & \dfrac{9.396 \text{ g$\cdot$mol}^{-1}}{M}\\\\M& = & \dfrac{9.405\text{ g$\cdot$mol}^{-1}}{0.07193}\\\\& = & \text{131 g$\cdot$mol}^{-1}\\\end{array}$

The molar mass is 131 g/mol, so the molecular mass is 131 u.

(d) Calculate the empirical formula

EF Mass = (12.01 + 1.008) u = 13.02 u

The molecular formula is an integral multiple of the empirical formula.

MF = (EF)ₙ

$n = \dfrac{\text{MF Mass}}{\text{EF Mass }} = \dfrac{\text{131 u}}{\text{13.02 u}} = 10.0 \approx 10$

MF = (CH)₁₀ = C₁₀H₁₀

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The empirical formula of a compound is ch. at 200 degrees celsius, 0.242 of this compound occupies 97.2ml at a pressure of 0.740atm. what is the molecular formula of the compound ?

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