Calculate ΔE for a process in which a system performs 4.34 kJ of work and absorbs 12.43 kJ of heat. Express your answer to two p
1 answer:
Answer:The change in internal energy , is 8.09 kJ
Explanation:
According to first law of thermodynamics:
=Change in internal energy
q = heat absorbed or released = +12.43 kJ (heat absorbed is positivew = work done or by the system = - 4.34 kJ (Work done by the system is negative)
Thus change in internal energy is 8.09 kJ
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Energy of wave depends on its amplitude and it is given as
here k = constant
A = amplitude
so energy will increase or decrease depends on the amplitude of the wave
So here if we need to check which wave has lower energy then we need to compare the amplitude.
If the amplitude is less then energy must be less
So please check in the figure that which wave out of A and B has lesser amplitude to find out the wave of lesser energy
Answer: D. the distance between the highest points of consecutive waves
Explanation:
The wavelength of a wave is defined as the <em>distance traveled by a periodic perturbation that propagates through a medium in a given time interval</em>. It is usually represented by and can be calculated if the frequency of the wave is known, since there is an inverse relationship between both.
In the specific case of a periodic sine wave (which is the way in which a wave is usually represented graphically) the wavelength can be determined as the distance between two consecutive maxima of the disturbance.
Therefore, the correct option is D.