- #1
ayans2495
- 58
- 2
- Homework Statement
- 100 g of ice at 0 ºC is added to an insulated chamber containing 20 g of steam at 100 ºC. What is the final temperature of the 120 g of water?
- Relevant Equations
- Q = mcΔT
Q = ml
The condensed steam loses heat, so the heat it loses is a positive quantity. This is in addition to the heat it yielded in condensing.ayans2495 said:That is exactly question. I would assume that it is negative though i didn't get the right answer with it. Maybe my math was wrong. On the contrary, as heat is extracted from the steam, I believe ΔT is negative.
It won't. You are making it far more complicated than the question setter would have intended.Alpher-Bethe-Gamow said:Some energy will be given to break bonds and forming bonds releases energy so that this is not an isothermal process, as the temperature in the closed system will change. If there were no changes in states of matter then you would be right, as the temperature change by one would directly be affected by the temperature change in the other. I hope this helps,
I know question setters sometimes ignore air resistance etc. but I don't think they will ignore the laws of thermodynamics :) Also the change of temperature is irrespective of direction in this equation, should point that out as it seems you want to look at that in your posts, 100 -> 50 is the same as 0 -> 50, no negatives used.haruspex said:It won't. You are making it far more complicated than the question setter would have intended.
Using which formula? The equation in post #1 has a sign error, as I indicated.ayans2495 said:I got a final temperature of 12 degrees Celsius using my formula, do you have the same?
It should be higher than 12, and haruspex is correct it should be a middling type of number,ayans2495 said:I got a final temperature of 12 degrees Celsius using my formula, do you have the same?
I'm really not sure what point you are making. All I see wrong in post #1 is a sign error.Alpher-Bethe-Gamow said:question setters sometimes ignore air resistance etc. but I don't think they will ignore the laws of thermodynamics
My interpretation of the equations in post #1 is that @ayans2495 is using T_{f} and T_{i} on the steam side (RHS) to mean the final and initial temperatures of the condensed steam respectively, the latter being 100C. So the T_{f}- T_{i} will produce a negative value. A positive one is needed.Alpher-Bethe-Gamow said:Also the change of temperature is irrespective of direction in this equation, should point that out as it seems you want to look at that in your posts, 100 -> 50 is the same as 0 -> 50, no negatives used.
Would i make the equation as followed:haruspex said:Using which formula? The equation in post #1 has a sign error, as I indicated.
Please post the equation you are now using and the subsequent working.
I get quite a bit more than 12C.
To get a feel for what the answer ought to be, note that although there is 5 times the mass of ice the latent heat of vaporisation is about seven times that of fusion, so it should be a middling sort of number.
You are right to assume this, and right in he needs to make it all positive, a simple adjustment, and he will have the answer!haruspex said:My interpretation of the equations in post #1 is that @ayans2495 is using T_{f} and T_{i} on the steam side (RHS) to mean the final and initial temperatures of the condensed steam respectively, the latter being 100C. So the T_{f}- T_{i} will produce a negative value. A positive one is needed.
What is the physical meaning of Q3?ayans2495 said:I thought so. This is great! Though would I need to do the same for Q3.
"Q3 is the amount of heat required to condensate the steam"ayans2495 said:Q3 is the amount of heat required to condensate the steam, as it is releasing heat one would think it is negative. On the contrary, there are no negative values in the equation Q=mlv, so I would suppose that it should be positive.
This came up just as posted, yes perfectly put.Steve4Physics said:"Q3 is the amount of heat required to condensate the steam"
No! No energy is required (i.e. you don't need to supply energy).
Have you ever boiled water to make a cup of tea? You *require* (must supply) an amount of energy ##ml_v## to convert water to steam.
But you do not need to supply any energy to condense the steam to water. In fact the steam *releases* an amount of energy ##ml_v## when it condenses.
In words, the equation ##Q_1 + Q_2 = Q_3 + Q_4## means:
Het required to melt ice
+ Heat required to raise ice from ##0^oC## to ##T_f##
=
Heat released when steam condenses
+
Heat released by condensed steam cooling from ##100^oC## to ##T_f##
Expressed this way, ##Q_1,Q_2, Q_3## and ##Q_4## must all be positive quanties.
I understood all that, thank you. I understand that to reverse the process energy is actually extracted from the steam, my English was just poor there. Again, thank you.Steve4Physics said:"Q3 is the amount of heat required to condensate the steam"
No! No energy is required (i.e. you don't need to supply energy).
Have you ever boiled water to make a cup of tea? You *require* (must supply) an amount of energy ##ml_v## to convert water to steam.
But you do not need to supply any energy to condense the steam to water. In fact the steam *releases* an amount of energy ##ml_v## when it condenses.
In words, the equation ##Q_1 + Q_2 = Q_3 + Q_4## means:
Het required to melt ice
+ Heat required to raise ice from ##0^oC## to ##T_f##
=
Heat released when steam condenses
+
Heat released by condensed steam cooling from ##100^oC## to ##T_f##
Expressed this way, ##Q_1,Q_2, Q_3## and ##Q_4## must all be positive quanties.
Thank you for your help and input, it really saved me.Alpher-Bethe-Gamow said:This came up just as posted, yes perfectly put.
Did you get a final temperature of 42 degrees Celsius.Steve4Physics said:Your original equation
##Q_1 + Q_2 = Q_3 + Q_4##
is based on ##Q_1, Q_2, Q_3## and ##Q_4## all being positive quantities.
##Q_4## is the thermal energy released when the water from the (condensed) steam cools from ##T_i = 100^oC## to ##T_f##.
You have used ##Q_4 = m_{steam} c_w (T_f - T_i)##
But ##T_i > T_f##, so ##T_f - T_i## will be negative and ##Q_4## will be negative, which is wrong.
So you need to make a 'manual adjustment' to allow for this, therefore use
##Q_4 = m_{steam} c_w (T_i – T_f)##
or
##Q_4 = -m_{steam} c_w (T_f – T_i)##
which then makes ##Q_4##, positive, as required.
Did you get a final temperature of 42 degrees Celsius.haruspex said:I'm really not sure what point you are making. All I see wrong in post #1 is a sign error.
My interpretation of the equations in post #1 is that @ayans2495 is using T_{f} and T_{i} on the steam side (RHS) to mean the final and initial temperatures of the condensed steam respectively, the latter being 100C. So the T_{f}- T_{i} will produce a negative value. A positive one is needed.
Yes.ayans2495 said:Did you get a final temperature of 42 degrees Celsius.
The final temperature of a mixture of ice and steam can be found by using the principle of energy conservation. This means that the total energy of the ice and steam before mixing must be equal to the total energy after mixing. By setting up an energy balance equation and solving for the final temperature, the exact value can be determined.
In order to find the final temperature of a mixture of ice and steam, you will need to know the initial temperatures of both substances, the mass of each substance, and the specific heat capacities of both ice and steam. These values are essential in setting up the energy balance equation and solving for the final temperature.
Yes, the final temperature of a mixture of ice and steam can be higher than 100 degrees Celsius. This is because the specific heat capacity of steam is much higher than that of ice, meaning that it requires more energy to raise the temperature of steam compared to ice. Therefore, when the two substances are mixed, the final temperature can exceed 100 degrees Celsius.
The mass of each substance has a direct impact on the final temperature of the mixture. The larger the mass of a substance, the more energy it contains. Therefore, if the mass of ice is greater than the mass of steam, the final temperature will be closer to the initial temperature of ice. On the other hand, if the mass of steam is greater, the final temperature will be closer to the initial temperature of steam.
No, it is not possible to find the final temperature without knowing the specific heat capacities of ice and steam. These values are essential in setting up the energy balance equation and solving for the final temperature. Without them, the calculation would be incomplete and the final temperature cannot be accurately determined.