How can the continuous addition of heat in a closed system cause it to explode?
2 answers:
Answer:
The heat builds pressure
Explanation:
Consider an ideal gas in a closed system (like a gas in a container: in this case, the volume of the gas is fixed). The ideal gas equation states that:
where
p is the gas pressure
V is the gas volume
n is the number of moles of the gas
R is the gas constant
T is the gas temperature
If heat is added to the gas, its temperature T increases. n and R are constant, and V is constant as well (the container does not change its volume), so this means that the pressure of the gas, p, increases as well. The more heat is added, the more the temperature increases, the more the pressure increase: at some point, the pressure against the internal walls of the container will become so strong that the container will explode.
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Answer:
Explanation:
We know that heat relates to mass, specific heat and variation of temperature experimented because of this heat through the equation . The heat released by the unknown material is absorbed by water, so we have
, and we can write:
Since thermal equilibrium is reached we know that , where we have added
to convert the temperature from Celsius to Kelvin, as <em>we must do</em>. Since we want the specific heat of the unknown material, we do:
Which for our values is: