A sample of hydrogen gas at a pressure of 0.520 atm and a temperature of 26.2°C, occupies a volume of 15.4 liters. If the gas is allowed to expand at constant temperature to a volume of 4.02 liters, the pressure of the gas sample will be atm.

1.99 atm

Explanation:

Step 1:

Data obtained from the question. This include the following:

Initial pressure (P1) = 0.520 atm

Initial temperature (T1) = 26.2°C

Initial volume (V1) = 15.4L

Final temperature (T2) = constant = 26.2°C

Final volume (V2) = 4.02L

Final pressure (P2) =..?

Step 2:

Determination of the new pressure of the gas.

Since the temperature of the gas is constant, it means the gas is obeying Boyle's law. Thus, the new pressure of the gas can be obtained by applying the Boyle's law equation as shown below:

P1V1 = P2V2

0.520 x 15.4 = P2 x 4.02

Divide both side by 4.02

P2 = (0.520 x 15.4) / 4.02

P2 = 1.99 atm

Therefore, the new pressure of the gas is 1.99 atm

out of these options:

ability to burn paper

pure sodium reacting violently with water

the boiling point of water

helium does not tend to react with anything

i would say this is a physical property:

helium does not tend to react with anything

why? :

i said helium does not tend to react with anything because well, it reacts to ! but ability to burn paper, pure sodium reacting violently with water, & the boiling point of water are chemical or

physical properties: the properties of a substance that can be observed without changing the chemical makeup of the substance

chemical properties: properties of a substance relating to the chemical nature and reactivity of the substance

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa