Answer:
Specific heat at constant pressure is = 1.005 kJ/kg.K
Specific heat at constant volume is = 0.718 kJ/kg.K
Explanation:
given data
temperature T1 = 50°C
temperature T2 = 80°C
solution
we know energy require to heat the air is express as
for constant pressure and volume
Q = m × c × ΔT ........................1
here m is mass of the gas and c is specific heat of the gas and Δ
T is change in temperature of the gas
here both Mass and temperature difference is equal and energy required is dependent on specific heat of air.
and here at constant pressure Specific heat is greater than the specific heat at constant volume,
so the amount of heat required to raise the temperature of one unit mass by one degree at constant pressure is
Specific heat at constant pressure is = 1.005 kJ/kg.K
and
Specific heat at constant volume is = 0.718 kJ/kg.K
Answer:
m = image distance/object distance
m=35/15=7/3
f=uv/(u+v)
35*15/(35+15)
f=10.5cm
Answer:
The remaining air between the cup and the rough surface exert pressure on the inner wall of the cup, due to this it does not stick on the rough surface.
Explanation:
HOPE it helps:))))
Answer:
As the can heats, the compressed gases will expand, causing the can to explode
Explanation:
We know that the gases in the aerosol can would assume the shape and volume of the can. The volume of the can would be the volume of the compressed gas.
As heat is added to the can, the aerosol gases would gain kinetic energy and their speed would increase. The gases would begin to expand and would require more space in order to move. This would indirectly increase the pressures between gas molecules and the walls of the can as collisions soars.
A point would eventually be reached where the gas agitation would lead to an explosion.
Overheated aerosol cans would explode.
