Final answer:
Without the mass of the iron, it's impossible to provide the specific heat of iron accurately. The formula q = mcΔT requires the mass to calculate the specific heat, which is not provided in the question.
Step-by-step explanation:
To calculate the specific heat of iron, you can use the formula q = mcΔT, where q is the heat absorbed or released, m is the mass, and ΔT is the change in temperature. The question provides the change in temperature and the heat released when a sample of iron cools down. Since the iron is releasing heat, q will be negative.
First, determine the change in temperature (ΔT): ΔT = Tfinal - Tinitial = 25.0°C - 50.4°C = -25.4°C (note that ΔT is negative because the temperature decreases).
We are given q = -197.0 J (negative because the heat is released) and the mass m is not given in the question. Assuming the mass is x grams, the formula becomes: -197.0 J = x g × specific heat × -25.4°C. To isolate the specific heat, divide both sides by -x g × -25.4°C. If the mass of the iron is provided, you can plug it into the formula to calculate the specific heat. Unfortunately, without the mass, it's impossible to determine the specific heat in J/g°C accurately.
In this particular question, the lack of the mass value of iron makes it impossible to provide the specific heat of iron.