Advertisements
Advertisements
Question
A 100 kg lock is started with a speed of 2.0 m s−1 on a long, rough belt kept fixed in a horizontal position. The coefficient of kinetic friction between the block and the belt is 0.20. (a) Calculate the change in the internal energy of the block-belt system as the block comes to a stop on the belt. (b) Consider the situation from a frame of reference moving at 2.0 m s−1 along the initial velocity of the block. As seen from this frame, the block is gently put on a moving belt and in due time the block starts moving with the belt at 2.0 m s−1. calculate the increase in the kinetic energy of the block as it stops slipping past the belt. (c) Find the work done in this frame by the external force holding the belt.
Advertisements
Solution
Here,
m = 100 kg
u = 2.0 m/s
v = 0
μk = 0.2
a) Internal energy of the belt-block system will decrease when the block will lose its KE in heat due to friction. Thus,
KE lost = `1/2m u^2-1/2mnu^2`
`1/2m(u^2-nu^2)`
`1/2xx100xx(2^2-0^2)`
= 200 J
b) Velocity of the frame is given by
uf = 2.0 m/s
u’ = u - uf = 2 – 2= 0
v’ = 0 – 2 = -2 m/s
KE lost = `1/2m u'^2-1/2mnu'^2`
`=1/2m(0^2-nu'^2)`
`=1/2xx100xx(0^2-2^2)`
= 200 J
c) Force of friction is given by
`f=mu_k^""R`
`rArrf=0.2xxmg=0.2xx100xx10=200N
`"Retardation"=f/m=200/100=2ms^-2`
Distance moved by the block will be as seen from the frame = s
`nu'^2-u'^2=2as`
`rArr2^2-0^2=2xx2s`
`rArrs=1"m"`
Work done by the force responsible for accelaration as seen from the frame = fs
= 200 x 1 = 200J
Work done by the belt to give it a final velocity of 2 m/s
`=1/2mnu'^2`
`=1/2xx100xx(2)^2`
= 200J
Total work done by external force as seen from the frame 200 + 200 = 400J
APPEARS IN
RELATED QUESTIONS
When we rub our hands they become warm. Have we supplied heat to the hands?
When a tyre bursts, the air coming out is cooler than the surrounding air. Explain.
Figure shows two processes A and B on a system. Let ∆Q1 and ∆Q2 be the heat given to the system in processes A and B respectively. Then ____________ .

Consider the following two statements.
(A) If heat is added to a system, its temperature must increase.
(B) If positive work is done by a system in a thermodynamic process, its volume must increase.
Which of the following system freely allows the exchange of energy and matter with its environment?
When does a system lose energy to its surroundings and its internal energy decreases?
A system releases 100 kJ of heat while 80 kJ of work is done on the system. Calculate the change in internal energy.
One gram of water (1 cm3) becomes 1671 cm3 of steam at a pressure of 1 atm. The latent heat of vaporization at this pressure is 2256 J/g. Calculate the external work and the increase in internal energy.
derive the relation between the change in internal energy (∆U), work is done (W), and heat (Q).
An ideal gas is compressed at a constant temperature. Its internal energy will ____________.
In a thermodynamic system, working substance is ideal gas. Its internal energy is in the form of ______.
8 m3 of a gas is heated at the pressure 105 N/m2 until its volume increases by 10%. Then, the external work done by the gas is ____________.
When 1 g of water at 0° C and 1 x 105 N/m2 pressure is converted into ice of volume 1.082 cm3, the external work done will be ____________.
Two samples A and B, of a gas at the same initial temperature and pressure are compressed from volume V to V/2; A isothermally and B adiabatically. The final pressure of A will be ______.
Two cylinders A and B of equal capacity are connected to each other via a stopcock. A contains a gas at standard temperature and pressure. B is completely evacuated. The entire system is thermally insulated. The stopcock is suddenly opened. Answer the following:
What is the final pressure of the gas in A and B?
In insulated systems, the amount of external work done by the gas is proportional to:
In thermodynamics, heat and work are ______.
The internal energy of one mole of argon is ______.
A system releases 125 kJ of heat while 104 kJ work is done on the system. Calculate the change in internal energy.
