Let's say I have a compound that melts at 50 degrees Celsius.
Case1 : I put it in a beaker of water at 100 degrees celsius (this is the temp of the H2O).
Case2 : Let's say I put it in a beaker of water at 90 degrees celsius (this is the temp of the H2O).
This is what I want to know.
I believe that JUST based off of Q=mc(Delta T) that would mean in case 2, MORE time would be required to melt the compound, because more heat would be needed. Please correct me if I'm wrong. Q has the units of Joules, thus meaning PER second, so if I were to decrease the time, I am decreasing the HEAT RATE.
However, would the TIME that the compound takes to melt be DIFFERENT in EITHER case depending on how much water I put in the beaker?
So if I put 500 grams as opposed to 200 grams, that would instead INCREASE the heat rate and THUS speed up the melting process. Is that right?
Case1 : I put it in a beaker of water at 100 degrees celsius (this is the temp of the H2O).
Case2 : Let's say I put it in a beaker of water at 90 degrees celsius (this is the temp of the H2O).
This is what I want to know.
I believe that JUST based off of Q=mc(Delta T) that would mean in case 2, MORE time would be required to melt the compound, because more heat would be needed. Please correct me if I'm wrong. Q has the units of Joules, thus meaning PER second, so if I were to decrease the time, I am decreasing the HEAT RATE.
However, would the TIME that the compound takes to melt be DIFFERENT in EITHER case depending on how much water I put in the beaker?
So if I put 500 grams as opposed to 200 grams, that would instead INCREASE the heat rate and THUS speed up the melting process. Is that right?