A system delivers 225 j of heat to the surroundings while delivering 645 j if work calculate the change in the internal Chang
2 answers:
The change in the internal energy:<u>-870 J</u>
<h3>Further explanation </h3>The laws of thermodynamics 1 state that: energy can be changed but cannot be destroyed or created
The equation is:
Energy owned by the system is expressed as internal energy (U)
This internal energy can change if it absorbs heat Q (U> 0), or releases heat (U <0). Or the internal energy can change if the system does work or accepts work (W)
The sign rules for heat and work are set as follows:
• The system receives heat, Q +
• The system releases heat, Q -
• The system does work, W -
• the system accepts work, W +
Heat can be calculated using the formula:
Q = mc∆T
A 225 Delivers System J Of Heat To The Surroundings While Delivering 645 J Of Work, then
Q release heat = -225 J
The system does work, W = -645 J
the change in the internal energy, ∆E, of the system
∆E / ∆U = Q + W
∆E / ∆U = -225 - 645
∆E / ∆U = -870 J
<h3>Learn more </h3>
the difference between temperature and heat
Specific heat
relationships among temperature, heat, and thermal energy.
When heat is added to a substance
You might be interested in
Answer 1) : The density of the hot air inside the balloon can be found out by using ideal gas equation;
PV = nRT;
As n is number of moles and in gases, number of moles along with mass per mole is equal to the density of the gas.
If the moles in the gas are more the density will be more.
here, density (ρ) = mass (m) / volume (V); substituting in the ideal gas equation we get,
ρ = mP / RT
Answer 2) ρ (hot air) = ρ (cold air) X
Here according to the formula because T(hot air) >T(cold air),
So, the density of hot air greater than the density of cold air.
The relationship between the ρ (h) = ρ(c) X