Question

five-gram samples of copper and iron are at room temperature. both samples receive equal amounts of energy due to heat flow. the specific heat capacity of copper is 0.09 cal/g°c, and the specific heat capacity of iron is 0.11 cal/g°c. which of the following statements is true? the temperature of each sample will increase by the same amount. the temperature of each sample will decrease by the same amount. the copper will get hotter than the iron. the iron will get hotter than the copper.

Answer 1

The copper will get hotter than the iron.

Step-by-step explanation:

Five-gram samples of copper and iron are at room temperature. Both samples receive equal amounts of energy due to heat flow. The specific heat capacity of copper is 0.09 cal/g°C, and the specific heat capacity of iron is 0.11 cal/g°C. Which of the following statements is true?

The temperature of each sample will increase by the same amount.

The temperature of each sample will decrease by the same amount.

The copper will get hotter than the iron.

The iron will get hotter than the copper.

Answer 2

Answer: the copper will get hotter than the iron.

Step-by-step explanation:
`Q= m* c* \Delta T`

Q= heat gained

m= mass of the substance

c = heat capacity

`\Delta T={\text{Change in temperature}}={\text{Final temperature- initial temperature}}`

Given
`q_(iron)=q_(copper)`
`m_(iron)=m_(copper)=5g` , also
`T_i{iron}=T_i{copper}=T_i`

we can write,
`c_(iron)(T_f{iron}-T_i)=c_(copper)(T_f{copper}-T_i)`

Thus as the two sides must be equal, the one having higher heat capacity must have lower final temperature. Ans as heat capacity of iron (0.11 cal/g°C) is higher than that of steel (0.09 cal/g°C), the final temperature of iron must be less and the copper will get hotter than the iron.