Calculate the enthalpy change for the melting of a 30 g ice cube. Show all your steps.
Any help is appreciated! :)
The heat of melting is well known.
Heatchange=Hmelting*mass
Sure! I'd be happy to help you with that. To calculate the enthalpy change for the melting of a 30 g ice cube, you will need to consider the heat energy required to melt the ice.
Here are the steps:
Step 1: Determine the heat energy required to raise the temperature of the ice from its initial temperature to its melting point.
The specific heat capacity of ice is approximately 2.09 J/g°C. Let's assume the initial temperature of the ice is -20°C and the melting point of ice is 0°C.
The equation to calculate the heat energy for this step is:
Q1 = mass × specific heat capacity × change in temperature
= 30 g × 2.09 J/g°C × (0°C - (-20°C))
Step 2: Determine the heat energy required to melt the ice at its melting point.
The heat of fusion for ice is approximately 334 J/g.
The equation to calculate the heat energy for this step is:
Q2 = mass × heat of fusion
= 30 g × 334 J/g
Step 3: Calculate the total heat energy (enthalpy change) for the melting of the ice.
The total heat energy is the sum of the heat energy for both steps.
Enthalpy change = Q1 + Q2
Step 4: Plug in the values and calculate the enthalpy change.
Enthalpy change = (30 g × 2.09 J/g°C × (-20°C)) + (30 g × 334 J/g)
I hope this helps! Let me know if you have any further questions.
Sure! To calculate the enthalpy change for the melting of a 30 g ice cube, we need to consider the heat transfer involved in the process. The enthalpy change, denoted as ΔH, can be obtained using the equation:
ΔH = q / m
where q is the heat transferred and m is the mass of the substance.
In this case, we need to determine the heat transfer q. To do that, we need to know the specific heat capacity of ice, denoted as c. The specific heat capacity of ice is approximately 2.09 J/g°C.
First, we need to calculate the heat required to raise the temperature of the ice cube from its initial temperature, T_initial, to its melting point, T_melting. The equation for that is:
q1 = m * c * (T_melting - T_initial)
Since we are assuming the ice cube starts at 0°C (T_initial = 0°C) and it melts at its melting point of 0°C (T_melting = 0°C), the equation simplifies to:
q1 = m * c * (0 - 0) = 0
Therefore, no heat is required to raise the temperature of the ice cube to its melting point.
Next, we need to calculate the heat required to melt the ice cube at its melting point. The equation for that is:
q2 = m * ΔH_fus
where ΔH_fus is the enthalpy of fusion of ice. The enthalpy of fusion of ice is approximately 334 J/g.
Substituting the values into the equation:
q2 = 30 g * 334 J/g
q2 = 10,020 J
Finally, we can calculate the total heat transfer, which is the sum of q1 and q2:
q = q1 + q2
q = 0 + 10,020 J
q = 10,020 J
Therefore, the enthalpy change for the melting of a 30 g ice cube is 10,020 J.