To what temperature should the oxygen at $27^{o} C$ be heated at constant pressure, so that the root man square velocity of its molecules becomes thrice of its previous value.

2700^{o} C

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2700 K

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2327^{o} C

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270 K

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Solution

The correct option is B $2700 K$
$v_{r m s} = \sqrt{\frac{3 R T}{M}}$
$T =$ temperature in Kelvin
$v_{r m s} \propto \sqrt{T}$

$\frac{v_{f}}{v_{i}} = \sqrt{\frac{T_{f}}{T_{i}}}$

$3 = \sqrt{\frac{T}{300}}$
Dividing both the equations we get
$T = 2700 K$

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To what temperature should the oxygen at 27oC be heated at constant pressure, so that the root man square velocity of its molecules becomes thrice of its previous value.

The correct option is B 2700 Kvrms=√3RTMT= temperature in Kelvinvrms∝√Tvfvi=√TfTi3=√T300Dividing both the equations we getT=2700K

To what temperature should the oxygen at $27^{o} C$ be heated at constant pressure, so that the root man square velocity of its molecules becomes thrice of its previous value.

The correct option is B $2700 K$
$v_{r m s} = \sqrt{\frac{3 R T}{M}}$
$T =$ temperature in Kelvin
$v_{r m s} \propto \sqrt{T}$

$\frac{v_{f}}{v_{i}} = \sqrt{\frac{T_{f}}{T_{i}}}$

$3 = \sqrt{\frac{T}{300}}$
Dividing both the equations we get
$T = 2700 K$