Figure 1 shows a small piece of copper about 3 cm high - Edexcel - GCSE Physics Combined Science - Question 1 - 2020 - Paper 1

To calculate the density of copper, use the formula:

$\text{Density} = \frac{\text{mass}}{\text{volume}}$

Given:

• Mass of copper, $m = 0.058 \, \text{kg}$
• Volume of copper, $V = 6.5 \times 10^{-6} \, \text{m}^3$

Substituting the values into the formula:

$\text{Density} = \frac{0.058}{6.5 \times 10^{-6}}$

Calculating this gives:

$\text{Density} = 8923.08 \, \text{kg/m}^3 \approx 8900 \, \text{kg/m}^3$

Using the equation:

$\Delta Q = m \times c \times \Delta T$

Given:

• Energy gained by cold water, $\Delta Q = 1050 \, \text{J}$
• Mass of copper, $m = 0.058 \, \text{kg}$
• Temperature change, $\Delta T = 22 - 100 = -78 \, \text{°C}$ (the temperature change is negative as the copper loses energy)

Rearranging the formula to find specific heat capacity, $c$:

$c = \frac{\Delta Q}{m \times \Delta T}$

Substituting the values:

$c = \frac{1050}{0.058 \times -78}$

Calculating this yields: $c \approx 230 \, \text{J/kg°C}$

1. Reduce Heat Loss: To minimize heat loss during the experiment, the student can insulate the glass beaker or cover it to maintain the temperature of the water. This would ensure that more accurate temperature measurements are obtained without loss of thermal energy.

2. Use More Accurate Measurement Tools: The student could use a more accurate thermometer or balance to ensure precise readings of temperature and mass, which would lead to more reliable calculations of specific heat capacity.