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?

1125mL

Explanation:

this can be done using general gas law

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:

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:

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:

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

Then

P2=1,125 torr

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

did anyone actually do this? like if anyone has submitted this i rly need .

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.