The density of acetic acid vapor at 300 K an | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The density of the gas is $\rho = 5 \ mg \ cm^{-3} = 5 \ g \ L^{-1}$.Using the ideal gas equation $pV = nRT$,where $n = \frac{w}{M}$,we have $p =

Vedclass · Accepted Answer

$2$

Vedclass · Answer

(B) The density of the gas is $ho = 5 \ mg \ cm^{-3} = 5 \ g \ L^{-1}$.Using the ideal gas equation $pV = nRT$,where $n = \frac{w}{M}$,we have $p = \frac{wRT}{MV} = \frac{ho RT}{M}$.Rearranging for the molar mass $M$ of the vapor cluster: $M = \frac{ho RT}{p}$.Given $ho = 5 \ g \ L^{-1}$,$R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$,$T = 300 \ K$,and $p = 1 \ atm$:$M = \frac{5 	imes 0.0821 	imes 300}{1} = 123.15 \ g \ mol^{-1}$.The molar mass of a single acetic acid molecule $(CH_3COOH)$ is $60 \ g \ mol^{-1}$.The number of molecules in the cluster is $n = \frac{M_{cluster}}{M_{monomer}} = \frac{123.15}{60} \approx 2.05$.Thus,the number of molecules is closest to $2$.

The density of acetic acid vapor at $300 \ K$ and $1 \ atm$ is $5 \ mg \ cm^{-3}$. The number of acetic acid molecules in the cluster that is formed in the gas phase is closest to

Similar Questions

At $300 \ K$,$22 \ g$ of $CO_2$ gas exerts a pressure of $5 \ atm$. What is the volume of the gas at the same temperature (in $dm^3$)? $(R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$

An open flask at $27^{\circ}C$ contains air. To what temperature $(^{\circ}C)$ should it be heated so that one-third of the air is expelled from the flask?

The temperature at which $4 \ mol$ of a gas occupies $5 \ dm^3$ volume at $3.32 \ bar$ pressure is:

If $P$ is pressure and $\rho$ is density of a gas,then $P$ and $\rho$ are related as

The gas equation $PV = nRT$ is applicable for which of the following conditions?

Vedclass Test Series

Exam Paper Generator

Online Exam Module