Question

A soda can was left out in the sun all day. Originally the can was at room temperature, 295 K, and had an internal pressure of 3.56 atm. If the temperature reduces to 280.92 K, what is the new pressure? A) 3.73 atm B) 2.89 atm C) 2.53 atm D) 4.01 atm

Answer 1

A soda can was left out in the sun all day, originally the can was at room temperature, 295 K, the new pressure in the can is approximately A. 3.37 atm.

Step-by-step explanation:

According to the ideal gas law, the pressure and temperature of a gas are directly proportional. This means that as the temperature increases, the pressure also increases, and vice versa.

To calculate the new pressure, we can use the formula:

P2 = (P1 * T2) / T1

Where

P2 is the new pressure

P1 is the original pressure

T2 is the new temperature

T1 is the original temperature.

Plugging in the values from the question, we get:

P2 = (3.56 atm * 280.92 K) / 295 K = 3.37 atm.

Therefore, the new pressure in the can is approximately 3.37 atm, which is closest to option A) 3.73 atm.