A steam engine's boiler completely converts 155 kg of water to steam. This process involves the transfer of 3.5 x 10^8 J by heat. If steam escaping a safety valve does 1.76 x 10^8 J of work against the outside atmosphere, what is the net internal energy of the water-steam system?
Do I need to use the mass and specific heat of water to find Q, or am I making this more complicated than it is?
10
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To find the net internal energy of the water-steam system, you will need to consider the heat transferred to the system and the work done by the system.
In this case, you are given the heat transferred (Q) as 3.5 x 10^8 J and the work done (W) as 1.76 x 10^8 J. The net internal energy (ΔU) can be calculated using the first law of thermodynamics:
ΔU = Q - W
where ΔU is the change in internal energy, Q is the heat transferred, and W is the work done.
In this equation, Q represents the heat transferred during the process. Since the boiler completely converts 155 kg of water to steam, we can assume that all the heat transferred is used to convert water to steam. Therefore, you don't need to consider the specific heat of water.
To find the net internal energy (ΔU), substitute the given values into the equation:
ΔU = 3.5 x 10^8 J - 1.76 x 10^8 J
After performing the subtraction, you will find the net internal energy of the water-steam system.