The temperature of 6.30 mol of an ideal monatomic gas is raised 18.0 k in an adiabatic process. what are (a) the work w done by the gas, (b) the energy transferred as heat q, (c) the change δeint in internal energy of the gas, and (d) the change δk in the average kinetic energy per atom?

a) The work done by the gas is , that means, work is done on the gas, not viceversa.

b) because it is an adiabatic process.

c)

d) per atom

Explanation:

First, for an ideal monoatomic gas we have: , This result can be experimentally verified or derived from statistical mechanics.

From which we can see that:

An adiabatic process is one in which no heat is transferred to or from the system, therefore the first law can be written as:

we can calculate as follows:

which follows from our first equation.

Thus the gas doesn't do any work, on the contrary, work is done on the gas to compress it.

As a monoatomic gas can only store energy in kinetic energy form, we have that the change in internal energy is related to the change in kinetic energy.

So:

answer; /// the amount of material dissolved in a measure of liquid(concentration) the above statement is (true); /// good luck

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.