Question

The specific heat of gold is 0.126 J/g°C. What mass of gold would change its temperature from 25.0 °C to 60.0 °C with the addition of 2825 J of heat energy? a 570 g b 641 g c 540 g d 610 g

Answer 1

The correct answer is option B, 641 g

Step-by-step explanation:

Answer 2

The amount of heat energy needed to increase the temperature of a substance by
`\Delta T` is given by:

`Q=m C_s \Delta T`
where m is the mass of the substance, Cs is its specific heat capacity and
`\Delta T` is the increase in temperature of the substance.

In this problem, we have a certain mass m of gold, with specific heat capacity
`C_s=0.126 J/g^(\circ)C`, to which we add Q=2825 J of energy. Its temperature increases by
`\Delta T=60-25=35 ^(\circ)C`. Therefore, if we re-arrange the previous equation, we can find the mass of the block of gold:

`m= (Q)/(C_s \Delta T) = (2825J)/(0.126\cdot 35)} =641 g`
So, the correct answer is B.