Question

At what temperature will 0.554 moles of helium gas occupy 11.30 liters at 1.95 atmospheres?

Also, what are the 4 gas laws, and what relationships do the represent?

Answer 1

Answer:

This is what we're given:

P (pressure), which is 1.95 atm

V(volume), which is 11.30 L.

n(number of moles), which is 0.554 moles of helium gas.

We have to find T, or temperature. To do this, we'll need to use the Ideal Gas Law, which is:

$PV = nRT$

Rearranging this equation to get temperature on one side, we get:\\ $T =\frac{PV}{nR}\\ \\

Pressure \: is \: in \: atm \: and \\ volume \: is \: in \: L . \: This \: tells \\ \: us \: that \: we'll \: need \: to \: \\ use \: the \: value \: of \: 0.08206 L atm/K \: mol \: for \: R \: the \: ideal \: gas \: constant.\\ \\ Plugging in all of the values, we can solve for temperature:

[tex]T =\frac{PV}{nR}\\ \\

T = (1.95 atm × 12.30 L) ÷

(0.654 mol × 0.0820575LatmK−1)

mol

[tex]T =\frac{PV}{nR} \\ \\

T =

\frac{ (1.95 atm × 12.30 L)}{(0.654 mol × 0.0820575LatmK−1)}$

$T = 447 K$

4 gas laws, and relationships do they represent

Boyle’s Law (PV law)

a. Volume of a GIVEN MASS OF GAS (mass is fixed) is inversely proportional to the Absolute pressure of the gas at constant Temperature.

b. Absolute pressure means pressure that is measured relative to Vacuum. Vacuum = 0 pressure. Thus, absolute pressure is measured relative to absolute 0.

c. Another way : PV = Constant. Thus, if you measure the Pressure and Volume at 3 different times, then P1 V1 = P2 V2 = P3 V3. In order to keep the product as a constant, whenever Pressure increases, the Volume will decrease.

Charle’s Law (VT Law)

a. Volume of a GIVEN MASS OF GAS (mass is fixed) is directly proportional to the Absolute Temperature at constant pressure.

b. When you measure the Temperature of a body on a scale in which 0 corresponds to Absolute 0, then the measured temperature is Absolute Temperature. Put simply, this refers to the Kelvin scale.

c. Absolute 0 is the temperature at which objects are at their lowest possible energy (Since Temperature is a measurement of the Kinetic energy of the atoms).

Gay Lussac Law (PT Law)

a. Pressure of a GIVEN AMOUNT OF MASS (mass is fixed) at constant volume is directly proportional to the absolute Temperature (that is, Kelvin Temperature).

b. Another way : P / T = Constant. P1 / T1 = P2 / T2 = P3 / T3.

Avogadro’s law (Vn law)

a. All the above laws were talking about relationships at fixed mass. So we needed a law which would relate mass with other quantities. This is Avogadro’s law.

b. It is a very straight forward law, if the amount of gas in a Container increases (that is, if the amount of matter increases), then the Volume of the gas increases which is very straight forward.

c. Volume is directly proportional to n (number of moles) or V/n = Constant.

Answer 2

Considering the Ideal Gas Law, at 485.05 °K 0.554 moles of helium gas will occupy 11.30 liters at 1.95 atmospheres.

On the other side, the 4 gas laws are Gay Lussac's law, Boyle's law, Charles' Law and Avogadro's law.

Ideal Gas Law

Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where:

• P is the gas pressure.
• V is the volume that occupies.
• T is its temperature.
• R is the ideal gas constant.  The universal constant of ideal gases R has the same value for all gaseous substances.
• n is the number of moles of the gas.

Temperature of helium

In this case, you know:

• P= 1.95 atm
• V= 11.30 L
• T= ?
• R=0.082 $\frac{atm L}{mol K}$
• n= 0.554 moles

Replacing in the Ideal Gas Law:

1.95 atm×11.30 L = 0.554 moles× 0.082 $\frac{atm L}{mol K}$× T

Solving:

T= (1.95 atm×11.30 L) ÷ (0.554 moles× 0.082 $\frac{atm L}{mol K}$)  

T= 485.05 K

Finally, at 485.05 °K 0.554 moles of helium gas will occupy 11.30 liters at 1.95 atmospheres.

Gay Lussac's law

Gay Lussac's law states that the pressure of the 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.

Boyle's law

Boyle's law says that volume is inversely proportional to pressure: if pressure increases, volume decreases; while if the pressure decreases, the volume increases.

Charles' Law

Charles' Law that the volume is directly proportional to the temperature of the gas: if the temperature increases, the volume of the gas increases; while if the temperature of the gas decreases, the volume decreases.

Avogadro's law

Avogadro's law states that the volume is directly proportional to the amount of gas: if the amount of gas increases, the volume will increase, while if the amount of gas decreases, the volume will decrease.

Summary

In summary, the 4 gas laws are Gay Lussac's law, Boyle's law, Charles' Law and Avogadro's law.

Learn more about the gas laws:

• https://brainly.com/question/4147359