Recent content by enth

LOL, thank you for the effort. I know its not much, but I click every commercial link here every time I get in...:P Well, for starters let's go your way. I assume that the blackened body is either water or a material containing waters heat conductivity properties. Regarding your previous...

Lol, actually I thought this is the easiest option. What did you mean that is easier then? :P

No no, I'm talking about an insulated bowl where the only contact is between the air and the surface of the water. Basically what I'm aiming for is what I suppose a classical thermodynamics problem per the scenario you suggested. My bowl is completley hypothetical and in perfect environment...

I think so, thank you. Ok, So now that I'm trying to figure out the rate at which the colder water gains heat from the environment, should I use this formula: Heat conduction Q/ Time = (Thermal conductivity) x (Area) x (Thot - Tcold)/Thickness ? (the bowl is 50cm in diameter and 10 cm...

A quick question. In this infinite room you mention, is the reason that all of the energy for evaporation comes from the air and not from air+water, is because we use more mass of air, thus say 1 ton of air at 25C (blown over the bowl) will contain more energy than 1 kg of water at 25C?

I see... Well, I suppose that the heat comes from the air. So, are you saying that in a room temperature if I evaporate half a cup of water by blowing air, the temperature of the remainding water would not change?

Ok, so if my scenario is unrealistic, what is a realistic scenario then(when the water isn't hot so it's not the source of the energy)? Why is it that when I'm in a room that shows around 25C on the thermometer and I blow a fan over a glass dish (or a towel) with little water- the water dissapears?

Ummm... But are you sure that the entire use of the formulas was correct? Don't we have two unknowns here? 'Change in temperature' and 'Heat added'? How can we equate Q(Heat Added) to the overall heat of the system (the vapor molecules)? One is only a part of the other. Thank you.

So... 22.57kj= 22570 j 22570(j)=10(g)*4.186(j)*X(C)? 22570/41.86=X x=539? I obviously screwed the conversion somewhere... PS-4.186 (j/g) is the specific heat of water... PS2- Uhh... Actually on second thought, I think that this is a misunderstanding problem and not a...

Hmm... Thank you, I think that I almost understand you. So if I want to know what the temperature of the (25C) water would be after 10g were evaporated, I should multiply the amount of water (0.01 kg) by the latent heat of evaporation (2257 kj/kg for water) which would give me the result of...

Thank you for your answers, but here is the thing that got me stuck- Vaporization occurs when the surface molecules of the water receive energy from the air, allowing them to escape. Latent heat of water vapor, as far as I understood (and please correct if I'm wrong) is the entire energy that...

Hello, So, I'm not much of a physicist but I thought that at least this question will be simple enough to answer with some internet browsing... though it seems apparently that I can't tell my left from my right... :P I have a bowl of water at room temperature (25 C). I blow at it with a...