in isothermal process q=-W does this mean that during isothermal process, amount of work done by tha system (-W) is equal to the amount of heat gained by the system(+q) if not what does it mean

Q. Assertion :For an isothermal reversible process $Q=-W$ i.e. work done by the system equals the heat absorbed by the system. Reason: Enthalpy change $\left(△H\right)$ is zero for isothermal process.

Q. For isothermal process, if heat added is $Q$ & work done by gas is $w$, then

Q. Let Q and W denote the amount of heat given to an ideal gas and the work done by it in an isothermal process.
(a) Q = 0
(b) W = 0
(c) Q ≠ W
(d) Q = W

Q. Let $Q$ and $W$ denote the amount of heat given to an ideal gas and the work done by it in an isothermal process.

Q. Express the change in internal energy of a system when

$i.$ No heat is absorbed by the system from the surroundings, but work $\left(w\right)$ is done on the system. What type of wall does the system have ?

$ii.$ No work is done on the system, but q amount of heat is taken out from the system and given to the surroundings. What type of wall does the system have?

$iii.$ w amount of work is done by the system and $q$ amount of heat is supplied to the system. What type of system would it be?