Question

A sample of hydrogen has an initial temperature of 50.°

c. when the temperature is lowered to -5.0° c, the volume of hydrogen becomes 212 cm3 . what was the initial volume of the hydrogen in dm3?

Answer 1

The initial volume of the hydrogen gas at 50.0 °C, after lowering the temperature to -5.0 °C and having a final volume of 212 cm^3, was 0.255 dm^3, calculated using Charles's law.

Step-by-step explanation:

The question involves the relationship between temperature and volume of a gas which is described by Charles's law. This law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature (in Kelvin) increases or decreases.

To find the initial volume of the hydrogen gas in dm3, we first convert the temperatures from Celsius to Kelvin by adding 273.15:

• Initial temperature: 50.0 °C = 50.0 + 273.15 = 323.15 K
• Final temperature: -5.0 °C = -5.0 + 273.15 = 268.15 K

The volume at -5.0°C is 212 cm3, which we convert to dm3 by dividing by 1000 (since 1 dm3 = 1000 cm3):

212 cm3 = 0.212 dm3

Now, applying Charles's law (V1/T1 = V2/T2), we can solve for the initial volume (V1):

V1 = V2 × (T1/T2)

V1 = 0.212 dm3 × (323.15 K / 268.15 K)

V1 = 0.212 dm3 × 1.2050

V1 = 0.255 dm3

The initial volume of the hydrogen was 0.255 dm3.

Answer 2

using the
V1/T1=V2/T2
where
T1=50C= 323.15K
T2= -5C=268.15 K
V2= 212m^3
substitute the given values, we will get the initial volume
V1=V2T1/T2
V1= 255.48m^3

The initial volume is 255.48m^3