Chemistry, 27.06.2019 23:40 luisannavasquez6129

If you doubled the volume of a sample of gas and
then doubled the volume again without changing
its pressure, how would the absolute temperature
of the gas be affected?
a
what pressure must be applied to keep a gas at
750 torr and 300 k at a constant volume of 200
ml if the temperature is raised to 450 k?

Answers: 2

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Answers

Answer from: luludawn2455

1125mL

Explanation:

this can be done using general gas law

If you doubled the volume of a sample of gas andthen doubled the volume again without changingits pr

Answer from: kylieweeks052704

The absolute temperature of the gas will be affected by a fourfold increase.

The pressure must be applied at 450 K should be 1,125 torr.

Explanation:

Charles's Law consists in the relationship between the volume and temperature of a certain amount of ideal gas, which is maintained at a constant pressure, by means of a constant of proportionality that is applied directly. For a given sum of gas at a constant pressure, as the temperature increases, the volume of the gas increases and when the temperature decreases, the volume of the gas decreases because the temperature is directly related to the energy of the movement of the gas molecules .

In summary, Charles's law is a law that says that when the amount of gas and pressure remain constant, the ratio between volume and temperature will always have the same value:

$\frac{V}{T} =k (constant)$

If you double the volume of a gas sample and then doubled the volume again, then the volume was increased four times. To comply with Charles's Law and maintain the relationship between volume and constant temperature, the temperature must increase four times, in the same way as volume.

So the absolute temperature of the gas will be affected by a fourfold increase.

Gay-Lussac's law can be expressed mathematically as follows:

$\frac{P}{T} =k$

Where P = pressure, T = temperature, K = Constant

This law indicates that the ratio between pressure and temperature is constant.

This law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of shocks against the walls increases, that is, the pressure increases. That is, the gas pressure is directly proportional to its temperature.

In short, when there is a constant volume, as the temperature increases, the gas pressure increases. And when the temperature decreases, gas pressure decreases.

When studying two different states of a gas, you have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment. When the temperature varies to a new T2 value, then the pressure will change to P2. This is true:

$\frac{P1}{T1} =\frac{P2}{T2}$

So in this case, as the volume is constant, Gay-Lussac's law can be applied as follows:

$\frac{750 torr}{300 K} =\frac{P2}{450 K}$

Then

$P2=\frac{750 torr}{300 K} *450 K\\$

P2=1,125 torr

The pressure must be applied at 450 K should be 1,125 torr.

Answer from: Quest

b) mutualism

hope this : )

Answer from: Quest

A) the enthralling of formation for pure element in its standard state is always positivehope this : )

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If you doubled the volume of a sample of gas and
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