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In a calorimeter with 200.0 g of water at 25.7 °C is 140 g of chromium metal placed at 73.0 °C. At a final temperature of 29.0 °C, the system achieves equilibrium. If the specific heat of water is 4.18 J/g·°C, what is the specific heat of the chromium metal in J/g·°C?
The temperature increases from 24.9°C to 43.6°C when 1.25 g of calcium metal reacts with 150 mL of 5.50 M aqueous HBr. If the heat capacity of the calorimeter is 769 J/°C, the specific heat of the final solution is 4.18 J/(g·°C), and the density of the solution is 1.00 g/mL, what is the ΔH in kJ/mol for the reaction?
A 1.00 g block of copper metal was heated to 95.0 °C. It was dropped in a coffee cup calorimeter containing 250.0 g of water at 24.5 °C. The temperature inside the cup changed to 34.9 °C after 1 hour. What is the heat released by the copper block? (specific heat copper = 0.385 J/g•°C)
Determine the heat released in the reaction if 9.78 g of rubidium hydroxide dissolved in 500.0 g of water with a temperature change of 25.0 °C to 78.0 °C.
