`(a)` Calculate the energy needed to raise the temperature of `10.0g` of iron from `25^(@)C` to `500^(@)C` if specific heat capacity of iron if `0.45J( .^(@)C)^(-1)g^(-1)`
`(b)` What mass of gold `(` of specific heat capacity `0.13J ( .^(@)C)^(-1)g^(-1)` can be heated can be heated through the same temperature difference when supplied with the same amount of energy as in `(a)` ?

Explanation

Mass of iron, `m=10.0 g`
Rise of temperature
`Deltat=500-25=475^(@)C` or `475 K`.
Specific heat capacity of iron,
`C=0.45 J(.^(@)C)^(-1) g^(-1)`
Energy needed `=mxxCxxDeltat`
`=10xx0.45xx475=2.1xx10^(3) J`
b. Specific heat capacity of gold`=0.13 J (.^(@)C^(-1))`
Energy `=mxxCxxDeltat`
`2.1xx10^(3)=mxx0.13xx475`
`(2.1xx10^(3))/(0.13xx475)=m`
`m=34 g`