Answer:
A. The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas.
D. As attractive forces between molecules increase, deviations from ideal behavior become more apparent at relatively low temperatures.
Explanation:
as we know by real gas equation
while ideal gas equation is given as
so from above formula we can say that net pressure is increased in real gas
Also we know that all real gas will close to behave like ideal gas when the pressure of the real gas is low and temperature of the gas is high
So above are the correct observations
Explanation:
Throughout this chapter, we have been studying traveling waves, or waves that transport energy from one place to another. Under certain conditions, waves can bounce back and forth through a particular region, effectively becoming stationary. These are called standing waves.
I would say its c
given a fixed volume, when volume decreases while mass remains constant
density increases ie temperature increases also
Can you write out the question please? :) Sorry, i don't see it on the paper
<u>Thermal energy</u><u> from the room-temperature water will continuously flow to the boiling water.</u>
- The second law states, in a straightforward manner, that heat cannot naturally go "uphill."
- When a pan of boiling water and a pan of ice are in touch, the hot water cools and the ice melts and warms up.
<h3>
THE FIRST LAW OF THERMODYNAMICS</h3>
- Adiabatic Process - is a procedure that is carried out without the system's heat content changing.
- Water is heated to a temperature of 1000C during the boiling process, making it an isothermal process. As steam, the excess heat leaves the system.
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