Question

A 200-gram sample of iron, initially at 0 degrees C, absorbs 660 calories of heat. Determine the final temperature attained by the iron sample if the specific heat capacity of iron is 0.11 cal/g degrees C.

Answer 1

To determine the specific heat of the unknown metal, we can use the heat formula: Q = mcΔT. Given that the temperature increases from 24.5 °C to 39.1 °C and the mass of the metal is 217 g, and the amount of heat absorbed is 1.43 kJ, we can substitute these values into the formula.

Step-by-step explanation:

To determine the specific heat of the unknown metal, we can use the heat formula: Q = mcΔT. Given that the temperature increases from 24.5 °C to 39.1 °C and the mass of the metal is 217 g, and the amount of heat absorbed is 1.43 kJ, we can substitute these values into the formula.

First, convert 1.43 kJ to joules by multiplying by 1000: 1.43 kJ * 1000 J/kJ = 1430 J.

Next, substitute the values into the formula: 1430 J = (217 g) * (specific heat) * (39.1 °C - 24.5 °C).

Solve for the specific heat of the metal by rearranging the formula: specific heat = 1430 J / (217 g * (39.1 °C - 24.5 °C)). This will give you the specific heat of the metal in J/g°C.