Question

describe an experiment to determine the volume coefficient of air at constant pressure.​

Answer 1

${ \mathfrak{ \overline{ \underline{ \red{ INTRODUCTION }}}}}$

This test is based on the investigation of the equilibrium of air expansion using a simple laboratory built; the stopper flask method, where the pressure resides throughout the study. The increase in gas volume is proportional to the increase in its temperature and is expressed as a fraction of the magnitude of the change in unit temperature. The air will evaporate easily when heated and then enters the contract when it has cooled.

The purpose of the trial was to:

* Find the corresponding amount of air expansion using the default flask method.

The bottle was suspended and a thick tube allowed contact with the outside. The bottle was heated with a beaker (with water) and then quickly transferred to cold water where cold water was allowed to enter and the air inside the bottle went down. The initial and final values of air and water are calculated (directly or indirectly - whichever is applicable) and the coefficient is calculated from this.

Its design test allowed for the calculation of the air expansion equity of 3.22 * 10-3 K-1. This is calculated at a temperature of 24oC and a pressure of 1 atm, which provides a good estimate compared to the theoretical value of 3.37 * 10-3 at a temperature of 24 oC (297 K).

${ \mathfrak{ \overline{ \underline{ \red{ THOUGHT }}}}}$

Dooley (1919) points out that gases are said to be completely elastic because they are infinite and elastic and form a contraction under the action of heat. That is, everything when in a gas state and not close to its exposure area has the same amount of expansion, the coefficient of 1/273 of its volume per degree Centigrade.

He goes on to say that as a gas enters 1/773 part of its capacity when its temperature is reduced by 1 ° C, such an excessive reduction can reduce its volume to zero at a temperature of 273 ° C. for this low temperature to be obtained, however, no such reduction is present. At the same time, it can be said that if the temperature is considered to be the movement of molecules of an object, that movement will be considered complete when the temperature reaches - 273 ° C.

This is the equivalent of a good gas expansion.

${ \mathfrak{ \overline{ \underline{ \red{ GAY \: LUSSACS \: LAW }}}}}$

Madan (2008: 81) shows that the equilibrium amount of the expansion of an object at any given temperature, t, is a small fraction of its volume which will grow one centimeter of that cell when heated from it.

* Gases are affected by changes in temperatures in general, such as liquid and solidarity, which increase when heated and are absorbed when cooled.

* With a given temperature change, they change in volume at a much higher rate than liquid or solid.

* All gases, at temperatures above their melting points, have the same amount of elasticity. This was first seen by Gay Lussac and Charles, and is very remarkable, and very different from what has been observed in the case of solids and liquids, each with its own special coefficient of expansion, which is often very different from those of others.

${ \mathfrak{ \overline{ \underline{ \red{ CONTINUED\: INCREASE \:IN \:PRESSURE }}}}}$

Atkins (2006: p35) shows that:

By definition:

With constant pressure:

This indicates that the work performed is actually the difference between the final and first volume multiplied by the (constant) unit of pressure. Once you can say that the gas expands (independent of pressing) but depends on the temperature as provided by:

${ \mathfrak{ \overline{ \underline{ \red{ HOW }}}}}$

By the way the hand was made, however, a small water-based bucket was used to heat the flask and then atmospheric pressure was used instead of studying the barometric (which was not available).