When the bulb of a constant-volume gas thermometer is placed in a beaker of boiling water at 100°C, the pressure of the gas is 223 mmHg. When the bulb is moved to an ice-salt mixture the pressure of the gas drops to 159 mmHg. Assuming ideal behavior, as in the figure below, what is the Celsius temperature of the ice-salt mixture?
When the bulb of a constant-volume gas thermometer is placed in a beaker of boiling water at 100°C?
Well, there is no "figure below," but maybe we can solve it anyway.
P1 / T1 = P2 / T2 (Gay-Lussac's Law)
T2 = (P2)(T1) / P1 = (159 mm)(373 K) / 223 mm = 266 K
Temperature = 266 K -273 = -7 degrees Celsius
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