A hot lump of 35.8 g of copper at an initial temperature of 70.7 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to
reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
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Answer:
New volume, v2 = 0.8L
Explanation:
<u>Given the following data;</u>
Original Volume = 2L
Original Temperature = 280K
New Temperature = 700K
To find new volume V2, we would use Charles' law.
Charles states that when the pressure of an ideal gas is kept constant, the volume of the gas is directly proportional to the absolute temperature of the gas.
Mathematically, Charles is given by;
Making V2 as the subject formula, we have;
V2 = 0.8L
Therefore, the volume of the gas after it is heated is 0.8L.