Calorimetry — MCQ Practice

A 2.0 g sample of a substance is heated from 20°C to 30°C, absorbing 40 J of heat. What is the specific heat capacity of the substance?

When 50 mL of 1.0 M HCl is mixed with 50 mL of 1.0 M NaOH in a coffee-cup calorimeter, the temperature of the solution increases from 25.0°C to 31.8°C. Assuming the density of the solution is $1.0 \text{ g/mL}$ and its specific heat capacity is $4.18 \text{ J/g}\cdot\text{°C}$, calculate the heat of neutralization (q) for the reaction.

A 10.0 g sample of an unknown metal at 100.0°C is placed in a coffee-cup calorimeter containing 50.0 g of water at 22.0°C. The final temperature of the water and metal is 24.5°C. What is the specific heat capacity of the metal? (Specific heat capacity of water = $4.184 \text{ J/g}\cdot\text{°C}$)

Which of the following statements about a bomb calorimeter is correct?

How much heat is released when 20.0 g of steam at 100°C condenses to liquid water at 100°C? (Latent heat of vaporization of water = $2260 \text{ J/g}$)

A reaction releases $1500\text{ J}$ of heat. If this heat is absorbed by a calorimeter with a heat capacity of $250 \text{ J/°C}$, what will be the temperature increase of the calorimeter?