It is a well-known fact that water has a higher specific heat than iron. Now, consider equal masses of water and iron that are initially in thermal equilibrium. The same amount of heat, 30 calories, is added to each one. Which statement is true?

A. They remain in thermal equilibrium

B. They are no longer in thermal equilibrium; the iron is warmer

C. They are no longer in thermal equilibrium; the water is warmer

D. It is impossible to say without knowing the exact mass involved

E. It is impossible to say without knowing the exact specific heats

Question

Ming

Physics

15 July, 04:39

It is a well-known fact that water has a higher specific heat than iron. Now, consider equal masses of water and iron that are initially in thermal equilibrium. The same amount of heat, 30 calories, is added to each one. Which statement is true?

A. They remain in thermal equilibrium

B. They are no longer in thermal equilibrium; the iron is warmer

C. They are no longer in thermal equilibrium; the water is warmer

D. It is impossible to say without knowing the exact mass involved

E. It is impossible to say without knowing the exact specific heats

+1

Answers (1)

Know the Answer?

Kaydence Combs · Answer 1

Answer:b

Explanation:

It is known that water has a higher value of specific heat as compared to iron, therefore, water requires high heat to raise the temperature of both water and iron by the same amount

If the same amount of heat is given to the same mass of different nature then iron will be warmer because its heat capacity is low so less heat can raise more temperature compared to water

Thus correct option is b