Answer:
The final temperature will be 3600 K.
Explanation:
Side 1
T=927°C
T=1200 K
Lets take volume of one side is V then the volume of other side will be 2V. The final volume of system will become 3 V.
The system is closed so the mass of system will remain constant .
We know that for ideal gas P V = m R T
The final pressure is same as initial pressure so we can say that
So the final temperature will be 3600 K.
The change in the player's internal energy is -491.6 kJ. The number of nutritional calories is -117.44 kCal
For this process to take place, some of the basketball player's perspiration must escape from the skin. This is because sweating relies on a physical phenomenon known as the heat of vaporization.
The heat of vaporization refers to the amount of heat required to convert 1g of a liquid into a vapor without causing the liquid's temperature to increase.
From the given information,
The amount of heat loss is represented by dQ.
where;
∴
Using the first law of thermodynamics:b
dU = dQ - dW
dU = -mL - dW
dU = -(0.110 kg × 2.26 × 10⁶ J/kg - 2.43 × 10⁵ J)
dU = -491.6 × 10³ J
dU = -491.6 kJ
The number of nutritional calories the player has converted to work and heat can be determined by using the relation:
dU = -117.44 kcal
Learn more about first law of thermodynamics here: