A constant volume thermometer registers a pressure of 1-500 - 104 Pa at the triple point of water and a pressure of 2-050 - 104 Pa at the normal boiling point- What is the temperature at the normal boiling point -

Given P_tr = 1.500 × 10^4 Pa P = 2.050 × 10^4 Pa We know, for constant volume gas thermometer T = P/P_tr× 273.16 K = 2.050 × 10^4/1.5 × 10^4× 273.16 = 373.31 ...

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Standard XII

Chemistry

Pressure and Temperature

A constant vo...

Question

A constant volume thermometer registers a pressure of $1.500 \times 10^{4}$ Pa at the triple point of water and a pressure of $2.050 \times 10^{4}$ Pa at the normal boiling point. What is the temperature at the normal boiling point ?

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Solution

Given $P_{t r} = 1.500 \times 10^{4} P a$

$P = 2.050 \times 10^{4} P a$

We know, for constant volume gas thermometer

$T = \frac{P}{P_{t r}} \times 273.16 K$

$= \frac{2.050 \times 10^{4}}{1.5 \times 10^{4}} \times 273.16$

= 373.31

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A constant volume thermometer registers a pressure of 1.500×104 Pa at the triple point of water and a pressure of 2.050×104 Pa at the normal boiling point. What is the temperature at the normal boiling point ?

Given Ptr=1.500×104 Pa P=2.050×104 Pa We know, for constant volume gas thermometer T=PPtr×273.16 K =2.050×1041.5×104×273.16 = 373.31

A constant volume thermometer registers a pressure of $1.500 \times 10^{4}$ Pa at the triple point of water and a pressure of $2.050 \times 10^{4}$ Pa at the normal boiling point. What is the temperature at the normal boiling point ?

Given $P_{t r} = 1.500 \times 10^{4} P a$

$P = 2.050 \times 10^{4} P a$

We know, for constant volume gas thermometer

$T = \frac{P}{P_{t r}} \times 273.16 K$

$= \frac{2.050 \times 10^{4}}{1.5 \times 10^{4}} \times 273.16$

= 373.31