A lightbulb contains Ar gas at a temperature of 295K and at a pressure of 75kPa. The light bulb is switched on, and after 30 minutes its temperature is 418 K. What is a numerical setup for calculating the pressure of the gas inside the light bulb at 418K?

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A lightbulb contains Ar gas at a temperature of 295K and at a pressure of 75kPa. The light bulb is switched on, and after 30 minutes its temperature is 418 K. What is a numerical setup for calculating the pressure of the gas inside the light bulb at 418K?

Assume the volume of the light bulb remains constant.

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Answer 1 · 2017-05-09T06:27:58

The assumption is quite reasonable.........

Explanation:

$\frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{2}}$ $P_1/T_1=P_2/T_2$ given constant $n$ $n$ , and constant $V$ $V$ , conditions that certainly obtain with a fixed volume light bulb.

And so $P_{2} = \frac{P_{1}}{T_{1}} \times T_{2}$ $P_2=P_1/T_1xxT_2$

$=(75*kPa)/(295*cancelK)xx418*cancelK$

$~=100*kPa$ .

Had the light bulb been sealed at normal pressure during its manufacture, what do you think might occur when it is operated?

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A lightbulb contains Ar gas at a temperature of 295K and at a pressure of 75kPa. The light bulb is switched on, and after 30 minutes its temperature is 418 K. What is a numerical setup for calculating the pressure of the gas inside the light bulb at 418K?

Assume the volume of the light bulb remains constant.

1 Answer

Explanation:

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