i am going crazy trying to figure this out. i just completed an experiment with heats of fusion and vaporization but for some reason i cant answer and explain this question
would 20.0g of steam at 100 degree celsius be enough to melt 20.0g of ice at 0 degrees celsius?
please break it down so i understand!
You're posting a question which I answered last night. If you don't understand that answer let me know what you don't understand (in detail) and we can go from there. But there is no point in answering more than once.
i did respond. at least i hope i did this is my frist time using this site. I don't understand the heat vap or heat fusion. am i multiplying the mass of steam by the literature value of heat vaporization (40.67 kj/mol)? and then doing the same for fusion (6.01)?
is this correct?
20gsteam * 40.67 = 813.4 (q1)
20gice *6.01 = 120.2 (q2)
q1(813.4) > q2(120.2)
if this s right where does the temperature vales have to do with this problem? and because steam is greater than ice im assuming the answer is yes?
so lost..
To determine if 20.0g of steam at 100 degrees Celsius would be enough to melt 20.0g of ice at 0 degrees Celsius, we need to compare the amount of energy (heat) required for each phase change.
First, let's calculate the amount of energy required to heat 20.0g of steam from 100 degrees Celsius to its boiling point. The specific heat capacity of water is approximately 4.18 J/g°C. So, the total heat energy required can be calculated using the formula:
Q = m * c * ΔT
where Q is the heat energy, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.
Substituting the values:
Q = 20.0g * 4.18 J/g°C * (100 - 100) °C
As the temperature remains constant (100 - 100 = 0), no heat energy is required for this step.
Next, we need to calculate the heat energy required for the phase change from steam to water. The enthalpy of vaporization for water is approximately 40.7 kJ/mol or 40.7 J/g.
Using the formula Q = m * ΔH, where ΔH is the enthalpy of vaporization:
Q = 20.0g * 40.7 J/g
Now, let's calculate the heat energy required to cool the water from its boiling point (100 degrees Celsius) to 0 degrees Celsius. Again, we can use the formula:
Q = m * c * ΔT
where Q is the heat energy, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.
Substituting the values:
Q = 20.0g * 4.18 J/g°C * (100 - 0) °C
Now, let's calculate the heat energy required for the phase change from ice to water. The enthalpy of fusion for water is approximately 334 J/g.
Using the formula Q = m * ΔH, where ΔH is the enthalpy of fusion:
Q = 20.0g * 334 J/g
So now we have calculated the heat energy required for each step. To determine if the given amount of steam is enough to melt the ice, we need to compare the total heat energy required for the steam (heating + phase change) with the total heat energy required for the ice (cooling + phase change).
Total energy required for the steam:
Q_steam = Q_vaporization + Q_heating = (20.0g * 40.7 J/g) + 0 J
Total energy required for the ice:
Q_ice = Q_fusion + Q_cooling = 20.0g * 334 J/g + (20.0g * 4.18 J/g°C * (100 - 0) °C)
Once you have calculated the total energy required for the steam and the total energy required for the ice, compare the two values. If the total energy for the steam is equal to or greater than the total energy for the ice, then the steam would be enough to melt the ice. Otherwise, it would not be sufficient.
I hope this breakdown helps you understand the process of determining if the given amount of steam is enough to melt the ice!