a gas exerts a pressure of 1.00 atm at 273 K. At what tempreture the gas exerts a pressure of 4.00 atm.

Chemistry

1 answer:

Diano4ka-milaya [45]2 years ago

8 0

Considering Gay-Lussac's law, a gas exerts a pressure of 4.00 atm at 1,092 K.

<h3>Gay-Lussac's law</h3>

Gay-Lussac's law states that the pressure of a gas is directly proportional to its temperature: when there is a constant volume, as the temperature increases, the pressure of the gas increases. And when the temperature is decreased, gas pressure decreases.

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

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

where P= pressure, T= temperature, k= Constant

This law states that the ratio of pressure to temperature is constant.

Studying an initial state 1 and a final state 2, it is fulfilled:

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

<h3>Final temperature</h3>

In this case, you know:

P1= 1 atm
T1= 273 K
P2= 4 atm
T2= ?

Replacing in Gay-Lussac's law:

$\frac{1 atm}{273 K}=\frac{4 atm}{T2}$

Solving:

$T2\frac{1 atm}{273 K}=4 atm$

$T2=\frac{4 atm}{\frac{1 atm}{273 K}}$

Finally, a gas exerts a pressure of 4.00 atm at 1,092 K.

Learn more about Gay-Lussac's law:

brainly.com/question/4147359

#SPJ1

You might be interested in

Carbon dioxide and helium which has a higher van der waals force of attraction between molecules

raketka [301]

Answer:

Carbon dioxide

Explanation:

Neither helium nor carbon dioxide has a molecular dipole, so their strongest van der Waals attractive forces are London forces.

Helium is a small spherical atom with only a two electrons, so its atoms have quite weak attractions to each other.

CO₂ is a large linear molecule. It has more electrons than helium, so the attractive forces are greater. Furthermore, the molecules can align themselves compactly side-by-side and maximize the attractions (see below).

For example. CO₂ becomes a solid at -78 °C, but helium must be cooled to -272 °C to make it freeze (that's just 1 °C above absolute zero).