Question

If 10 calorie of heat energy is added to a
system and the system does 5 calorie of
work on the surroundings. What is the
energy change of the system?​

Answer 1

Answer:

Heat absorbed, q=500cal

Work done by the system, w=−350cal

Applying the first law of thermodynamics,

ΔU=q+w=500+(−350)=150 calorie

Explanation:

plz mark me as brainiest

Answer 2

Concept:

• The first law of thermodynamics
• According to this law, energy can only be changed in form; it cannot be created or destroyed. Mass crossing the control boundary, external work, or heat transfer across the barrier are all examples of energy transfer for any system.

Given:

• Heat energy Q added to the system = 10 cal
• Heat energy is added to the system, so the value is positive
• Work done by the system W = -5 cal
• Work is done by the system, so it has a negative value

Find:

• The energy change of the system

Solution:

According to the first law of thermodynamics,

ΔU = Q+W

Where ΔU is the change in internal energy of the system, Q is the heat energy and W is the work done.

ΔU = 10+(-5) = 5 cal

The energy change in the system is 5 calories.

#SPJ1