Find the pressure of a CO_2 gas when 6.022 ti | vedclass

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(B) $1$. Calculate the number of moles $(n)$: $n = \frac{6.022 	imes 10^{22}}{6.022 	imes 10^{23}} = 0.1 \ mol$. $2$. Convert temperature to Kelvin:

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$1.231$

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(B) $1$. Calculate the number of moles $(n)$: $n = \frac{6.022 	imes 10^{22}}{6.022 	imes 10^{23}} = 0.1 \ mol$. $2$. Convert temperature to Kelvin: $T = 27 + 273 = 300 \ K$. $3$. Use the ideal gas equation $PV = nRT$,where $R = 0.08314 \ L \cdot bar \cdot K^{-1} \cdot mol^{-1}$. $4$. $P = \frac{nRT}{V} = \frac{0.1 	imes 0.08314 	imes 300}{2} = \frac{2.4942}{2} = 1.247 \ bar$. $5$. Given the options,the closest value is $1.231 \ bar$.

Find the pressure of a $CO_2$ gas when $6.022 \times 10^{22}$ molecules are placed in a $2 \ L$ vessel at $27 \ ^oC$ temperature. (in $bar$)

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