Problem: A volume of 115 mL of H2O is initially at room temperature (22.00 °C). A chilled steel rod at 2.00 °C is placed in the water. If the final temperature of the system is 21.20 °C, what is the mass of the steel bar? Use the following values:specific heat of water = 4.18 J/ (g ⋅ °C)specific heat of steel = 0.452 J/ (g ⋅ °C)Express your answer to three significant figures and include the appropriate units.The heat capacity of an object indicates how much energy that object can absorb for a given increase in that object's temperature. In a system in which two objects of different temperatures come into contact with one another, the warmer object will cool and the cooler object will warm up until the system is at a single equilibrium temperature.Note the difference between the terms molar heat capacity, which has units of J/ (mol ⋅ °C), and specific heat, which has units of J/ (g ⋅ °C).In this problem answers are requested to three significant digits for grading purposes. The true number of significant digits may be more or less.

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A volume of 115 mL of H2O is initially at room temperature (22.00 °C). A chilled steel rod at 2.00 °C is placed in the water. If the final temperature of the system is 21.20 °C, what is the mass of the steel bar? Use the following values:

specific heat of water = 4.18 J/ (g ⋅ °C)
specific heat of steel = 0.452 J/ (g ⋅ °C)

Express your answer to three significant figures and include the appropriate units.


The heat capacity of an object indicates how much energy that object can absorb for a given increase in that object's temperature. In a system in which two objects of different temperatures come into contact with one another, the warmer object will cool and the cooler object will warm up until the system is at a single equilibrium temperature.

Note the difference between the terms molar heat capacity, which has units of J/ (mol ⋅ °C), and specific heat, which has units of J/ (g ⋅ °C).

In this problem answers are requested to three significant digits for grading purposes. The true number of significant digits may be more or less.

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