Question

1. the specific heat of iron is 0.473 j/g°c and the specific heat of lead is 0.128 j/g°c. in order to raise the temperature of one gram of those metals by one degree celsius, (1pts) both metals require the same amount of energy. the iron requires more energy than the lead. the lead requires more energy than the iron. no correct answer is given

Explanation:

Step1: Recall specific heat formula

The energy required to change temperature is given by $Q = mc\Delta T$, where $m$ = mass, $c$ = specific heat, $\Delta T$ = temperature change.

Step2: Plug in values for iron

For 1g iron, $\Delta T=1^\circ\text{C}$, $c=0.473\ \text{J/g}^\circ\text{C}$:
$Q_{\text{iron}} = 1 \times 0.473 \times 1 = 0.473\ \text{J}$

Step3: Plug in values for lead

For 1g lead, $\Delta T=1^\circ\text{C}$, $c=0.128\ \text{J/g}^\circ\text{C}$:
$Q_{\text{lead}} = 1 \times 0.128 \times 1 = 0.128\ \text{J}$

Step4: Compare the two energies

$0.473\ \text{J} > 0.128\ \text{J}$, so iron requires more energy.

Answer:

the iron requires more energy than the lead.