A car tyre is filled with nitrogen gas at 35 | vedclass

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(D) Assuming the volume of the tyre remains constant, according to Gay-Lussac's Law, $P \propto T$ (where $T$ is in Kelvin).Given: $P_1 = 35 \ \psi$,

Vedclass · Accepted Answer

$70$

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(D) Assuming the volume of the tyre remains constant, according to Gay-Lussac's Law, $P \propto T$ (where $T$ is in Kelvin).Given: $P_1 = 35 \ \psi$, $T_1 = 27 + 273 = 300 \ K$, $P_2 = 40 \ \psi$.Using the formula $\frac{P_2}{P_1} = \frac{T_2}{T_1}$:$\frac{40}{35} = \frac{T_2}{300}$$T_2 = \frac{40 	imes 300}{35} = \frac{12000}{35} \approx 342.86 \ K$.Converting back to Celsius: $T_2(^{\circ} C) = 342.86 - 273 = 69.86^{\circ} C$.Rounding to the nearest integer, we get $70^{\circ} C$.

$A$ car tyre is filled with nitrogen gas at $35 \ \psi$ at $27^{\circ} C$. It will burst if pressure exceeds $40 \ \psi$. The temperature in $^{\circ} C$ at which the car tyre will burst is ............ (Rounded-off to the nearest integer)

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