A gas has a volume of 4.00 L at 0 degree C. What final temperature, in degrees C, is needed to cause the volume of the gas to change to 50L, if the amount of the gas and its pressure are not changed? (Please show your work to receive credit)



Answer :

Answer:

To determine the final temperature needed to cause the volume of the gas to change from 4.00 L to 50 L, we can use Charles's Law. Charles's Law states that for a given amount of gas at constant pressure, the volume of the gas is directly proportional to its temperature in Kelvin. The law can be expressed as:

1

1

=

2

2

T

1

V

1

=

T

2

V

2

where

1

V

1

 and

2

V

2

 are the initial and final volumes, respectively, and

1

T

1

 and

2

T

2

 are the initial and final temperatures, respectively.

Given:

Initial volume,

1

=

4.00

V

1

=4.00 L

Final volume,

2

=

50

V

2

=50 L

Initial temperature,

1

=

0

C

T

1

=0

C

First, we need to convert the initial temperature from degrees Celsius to Kelvin. The Kelvin temperature scale can be obtained by adding 273.15 to the Celsius temperature:

1

=

0

C

+

273.15

=

273.15

K

T

1

=0

C+273.15=273.15 K

Now, using Charles's Law, we can solve for the final temperature

2

T

2

:

1

1

=

2

2

T

1

V

1

=

T

2

V

2

Rearranging to solve for

2

T

2

:

2

=

1

×

2

1

T

2

=T

1

×

V

1

V

2

Substituting the known values:

2

=

273.15

K

×

50

L

4.00

L

T

2

=273.15 K×

4.00 L

50 L

2

=

273.15

K

×

12.5

T

2

=273.15 K×12.5

2

=

3414.375

K

T

2

=3414.375 K

Finally, convert the temperature back to degrees Celsius by subtracting 273.15 from the Kelvin temperature:

2

=

3414.375

K

273.15

=

3141.22

5

C

T

2

=3414.375 K−273.15=3141.225

C

Thus, the final temperature needed to cause the volume of the gas to change to 50 L is approximately

3141.22

5

C

3141.225

C.

Explanation: