Question

lead, water, sulfur, and arsenic have specific heats of 0.128, 4.184, 0.706, and 0.329 j g⁻¹ °c⁻¹, respectively. which of these would require the largest amount of heat to increase the temperature by 10.0 °c, assuming each sample was the same mass?
○ water
○ sulfur
○ lead
○ arsenic

Explanation:

Step1: Recall the heat formula

The formula for heat \( q \) is \( q = mc\Delta T \), where \( m \) is mass, \( c \) is specific heat, and \( \Delta T \) is temperature change.

Step2: Analyze the variables

Given \( m \) (same for all) and \( \Delta T = 10.0^\circ C \) (same for all), \( q \) is directly proportional to \( c \).

Step3: Compare specific heats

Specific heats: lead (\( 0.128 \, J \, g^{-1} \, ^\circ C^{-1} \)), water (\( 4.184 \, J \, g^{-1} \, ^\circ C^{-1} \)), sulfur (\( 0.706 \, J \, g^{-1} \, ^\circ C^{-1} \)), arsenic (\( 0.329 \, J \, g^{-1} \, ^\circ C^{-1} \)). Water has the highest \( c \), so it needs the most heat.

Answer:

A. water