I'm a little bit confused over the following inequality:

$$ dS > \frac{\delta Q_{irrev}}{T} $$

An infinitesimal change in entropy is defined in this way: $$ dS = \frac{\delta Q_{rev}}{T} $$

Such that $$ \frac{\delta Q_{rev}}{T} > \frac{\delta Q_{irrev}}{T} $$

And this would imply that $$ \delta Q_{rev} > \delta Q_{irrev} $$

I find this a little confusing, because I would argue that, for example, in order to raise a system from an initial temperature to a final temperature a certain, fixed amount of heat is needed, regardless whether the process is reversible or not. If the process is irreversible, heat is transfered less efficient, so more heat in total would be needed to supply the fixed amount to the system, thereby implying that: $$ \delta Q_{rev} < \delta Q_{irrev} $$

Can someone explain to me why my reasoning is wrong?

Thanks in advance

I'm a little bit confused over the following inequality:

$$ dS > \frac{\delta Q_{irrev}}{T} $$

An infinitesimal change in entropy is defined in this way: $$ dS = \frac{\delta Q_{rev}}{T} $$

Such that $$ \frac{\delta Q_{rev}}{T} > \frac{\delta Q_{irrev}}{T} $$

And this would imply that $$ \delta Q_{rev} > \delta Q_{irrev} $$

I find this a little confusing, because I would argue that, for example, in order to raise a system from an initial temperature to a final temperature a certain, fixed amount of heat is needed, regardless whether the process is reversible or not. If the process is irreversible, heat is transfered less efficient, so more heat in total would be needed to supply the fixed amount to the system, thereby implying that: $$ \delta Q_{rev} < \delta Q_{irrev} $$

Can someone explain to me why my reasoning is wrong?

I'm a little bit confused over the following inequality:

$$ dS > \frac{\delta Q_{irrev}}{T} $$

An infinitesimal change in entropy is defined in this way: $$ dS > \frac{\delta Q_{rev}}{T} $$

Such that $$ \frac{\delta Q_{rev}}{T} > \frac{\delta Q_{irrev}}{T} $$

And this would imply that $$ \delta Q_{rev} > \delta Q_{irrev} $$

I find this a little confusing, because I would argue that, for example, in order to raise a system from an initial temperature to a final temperature a certain, fixed amount of heat is needed, regardless whether the process is reversible or not. If the process is irreversible, heat is transfered less efficient, so more heat in total would be needed to supply the fixed amount to the system, thereby implying that: $$ \delta Q_{rev} < \delta Q_{irrev} $$

Can someone explain to me why my reasoning is wrong?

Thanks in advance

I'm a little bit confused over the following inequality:

$$ dS > \frac{\delta Q_{irrev}}{T} $$

An infinitesimal change in entropy is defined in this way: $$ dS = \frac{\delta Q_{rev}}{T} $$

Such that $$ \frac{\delta Q_{rev}}{T} > \frac{\delta Q_{irrev}}{T} $$

And this would imply that $$ \delta Q_{rev} > \delta Q_{irrev} $$

I find this a little confusing, because I would argue that, for example, in order to raise a system from an initial temperature to a final temperature a certain, fixed amount of heat is needed, regardless whether the process is reversible or not. If the process is irreversible, heat is transfered less efficient, so more heat in total would be needed to supply the fixed amount to the system, thereby implying that: $$ \delta Q_{rev} < \delta Q_{irrev} $$

Can someone explain to me why my reasoning is wrong?

Thanks in advance