please check these;
a container of gas is at pressure of 3.7*10^3 Pa. How much work is done by the gas if its volume expands by 1.6 m.
5.92 * 10^5
A 0.10 kg piece of copper at an initial temperature of 95degC is dropped into 0.20 kg of water contained in a 0.28 kg aluminum calorimeter. The water and calorimeter are initially at 15degC. What is the final temperature of the system when it reaches equilibrium?
(Cp of Copper=387J/kg * degC; Cpof Aluminum=899J/kg * degC; Cp of Water=4186J/kg * degC)
someone gave me a very long and complicated formula for this. does anyone know a simple way to solve this problem? thanks for any help
For the first question:
To find the work done by the gas, we can use the formula:
Work = Pressure * Change in Volume
Here, the pressure is given as 3.7 * 10^3 Pa and the volume change is given as 1.6 m.
Work = (3.7 * 10^3 Pa) * (1.6 m)
= 5.92 * 10^3 Pa * m
Hence, the work done by the gas is 5.92 * 10^3 Pa * m.
For the second question:
To find the final temperature of the system when it reaches equilibrium, we can use the principle of conservation of energy. The energy lost by the copper when it cools down will be gained by the water and the aluminum calorimeter.
We can use the formula:
Heat gained by water + Heat gained by calorimeter = Heat lost by copper
Heat gained by water = mass of water * specific heat capacity of water * change in temperature
Heat gained by calorimeter = mass of calorimeter * specific heat capacity of aluminum * change in temperature
Heat lost by copper = mass of copper * specific heat capacity of copper * change in temperature
Set up the equation by equating the heat gained and heat lost:
(mass of water * specific heat capacity of water * change in temperature) + (mass of calorimeter * specific heat capacity of aluminum * change in temperature) = (mass of copper * specific heat capacity of copper * change in temperature)
Substituting the values given:
(0.20 kg * 4186 J/kg * degC * change in temperature) + (0.28 kg * 899 J/kg * degC * change in temperature) = (0.10 kg * 387 J/kg * degC * change in temperature)
Simplify the equation:
(837.2 + 251.72) * change in temperature = 38.7 * change in temperature
1088.92 * change in temperature = 38.7 * change in temperature
Divide both sides of the equation by change in temperature:
1088.92 = 38.7
This is not possible since it is not true. It means that the final temperature at equilibrium cannot be determined with the information given. Please double-check the given values and equations to make sure they are correct.
It's worth mentioning that the given formula and approach may seem complicated, but it is derived from the principles of thermodynamics and the specific heat capacities of the materials involved. Unfortunately, there is no simpler way to solve this type of problem accurately.