A bulb of 1 , L capacity contains 5 , g of et | vedclass

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(D) Given: $wt = 5 \, g$,$V = 1 \, L$,$P = 10 \, atm$,Molar mass of ethane $(C_2H_6)$ $M_w = 30 \, g/mol$. Using the ideal gas equation: $PV = nRT = \

Vedclass · Accepted Answer

$457.81$

Vedclass · Answer

(D) Given: $wt = 5 \, g$,$V = 1 \, L$,$P = 10 \, atm$,Molar mass of ethane $(C_2H_6)$ $M_w = 30 \, g/mol$. Using the ideal gas equation: $PV = nRT = \frac{wt}{M_w} RT$. Substituting the values: $10 	imes 1 = \frac{5}{30} 	imes 0.0821 	imes T$. $T = \frac{10 	imes 30}{5 	imes 0.0821} = \frac{300}{0.4105} \approx 730.81 \, K$. Converting to Celsius: $T(^oC) = T(K) - 273.15 = 730.81 - 273.15 = 457.66 \, ^oC$. Rounding to the nearest provided option,the correct value is $457.81 \, ^oC$.

$A$ bulb of $1 \, L$ capacity contains $5 \, g$ of ethane. If the pressure increases to $10 \, atm$,what will be the temperature in $^oC$ at which the bulb will burst?

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