Question

Part B Check all the correct statements. Note: Push yourself to understand why these statements are true or false. If false think about an example that contradicts the statement, or think about how you would formulate the statement so it is correct. You will n you can answer a similar question that is formulated differently The internal energy of any gas (ie. not necessarily ideal) depends only the temperature of the system The kinetic energy of any gas (i.e. not necessarily ideal) depends only the temperature of the system O The internal energy of an ideal gas (those that obey PV nRT) equals the kinetic energy of its molecules The internal energy of 1 mole a real gas at moderate pressures is higher than the internal energy of 1 mole the same real gas at very low pressures. The temperature of the system is assumed to be the same The internal energy of an ideal gas (those that obey PV nRT) depends only the temperature of the system. The kinetic energy of 1 mole a real gas at moderate pressures is lower than the internal energy of 1 mole the same real gas at very low pressures. The temperature of the system is assumed to be the same

Answer 1

Answer :

In isothermal expansion of gases w < 0

Explanation: as w = -pdV

                       where p is pressure which is always positive, and in expansion dV ( infinitisimal small change in volume) is positive, which makes w < 0

Since at constant temperature (in isothermal processes) internal energy remains constant

and Change in internal energy = $\Delta$U = w + q = 0 so it gives w = -q or q = -w

and if w is less than zero and w = -q then consequently q must be greater than zero

So our answer is

q > 0, w < 0 and q = -w