Question

Chlorine gas has a pressure of 1.05 atm at 25°C. What pressure will it exert at 75°C?

Answer 1

The pressure of chlorine gas at 75°C is approximately 1.24 atm.

Step-by-step explanation:

To calculate the pressure of chlorine gas at 75°C, we can use the ideal gas law. According to the ideal gas law, the pressure of a gas is directly proportional to its temperature. So we can use the formula:

P1/T1 = P2/T2

Here, P1 is the initial pressure (1.05 atm), T1 is the initial temperature (25°C), P2 is the final pressure (unknown), and T2 is the final temperature (75°C). Rearranging the formula, we get:

P2 = P1 × (T2/T1)

Substituting the values, we get:

P2 = 1.05 atm × (75+273)/(25+273) = 1.24 atm

Therefore, the pressure of chlorine gas at 75°C is approximately 1.24 atm.

Answer 2

It will exert a pressure of 1.23 atm

Step-by-step explanation:

To calculate the pressure it will exert, we shall be using the Gay Lussac pressure law

Here, we know that pressure and volume are inversely proportional.

Mathematically:

P1/T1 = P2/T2

From the question, P1 = 1.05 atm

P2 = ?

T1 = 25 which when converted to Kelvin scale will be 25 + 273 = 298

T2 = 75 + 273 = 348

Plugging these values, we have;

1.05/298 = P2/348

= P2 = (348 * 1.05)/ 298 = 1.226 which is approximately 1.23 atm