For many purposes we can treat nitrogen (N,) as an ideal gas at temperatures above its boiling point of -196. °C. Suppose the temperature of a sample of nitrogen gas is raised from -25.0 °C to 11.0 °C, and at the same time the pressure is changed. If the
initial pressure
was 0.60 kPa and the volume decreased by 40.0%, what is the final pressure? Round your answer to 2 significant digits.
| kPa
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5
?

first let us lay out the formula for potential

and kinetic energy:

pe = mgh

ke = (mv^2)/2

where: m=mass, v=velocity, g=gravitational

acceleration, h=height

calculating for mass using the known values of

pe:

340j = m (9.81 m/s^2) (50ft) (1m/3.28ft)

m = 2.27 kg

the law of conservation of energy states that

energy is neither created nor destroyed. therefore, the change in kinetic

energy from 50 ft to 35 ft would be equal to the change in potential energy

from 50 ft to 35 ft. however it would be opposite in signs since one is losing

while other is gaining.

ke(35ft) – ke(50ft) = - [ pe(35ft) – pe(50ft]

ke(50ft) = 0 since the brick is initially at rest

ke(35ft) = 340j - 2.27kg (9.81 m/s^2) (35ft)

(1m/3.28 ft)

ke(35ft)

= 102.38 j

the answer is b. dilution