Question

a block of copper (cu) and a block of iron (fe) of identical mass are heated so that each receives exactly the same amount of heat transfer (+q). given the specific heat capacities of copper (0.386 j/g.°c) and iron (0.461 j/g.°c), which block will be at the higher temperature after the heating process? assume that no heat is lost to the surroundings. you dont need to do any calculations to solve this problem, just use the information provided by the specific heat capacities and understanding its units. the following may also be useful (but you shouldnt have to use them): q = cp·m·δt δt = q/cp·m copper iron dont test me yet, i am trying to gain an understanding before attempting to answer this question.

Explanation:

Step1: Analyze the formula for temperature change

The formula for heat transfer is \( q = C_p\cdot m\cdot\Delta T \). We can rearrange it to find \( \Delta T=\frac{q}{C_p\cdot m} \). Given that \( q \) (heat transfer) and \( m \) (mass) are the same for both copper and iron (since the blocks have identical mass and receive the same amount of heat), the temperature change \( \Delta T \) is inversely proportional to the specific - heat capacity \( C_p \).

Step2: Compare specific - heat capacities

The specific - heat capacity of copper \( C_{p,Cu}=0.386\ J/g\cdot^{\circ}C \) and of iron \( C_{p,Fe} = 0.461\ J/g\cdot^{\circ}C \). Since \( C_{p,Cu}

Answer:

Copper