What are the joules needed to melt 50.0g of ice at 0 degree C and to warm the liquid to 65.0 degree C?
Thank you so much!
To determine the total amount of heat required to melt the ice and raise the temperature of the resulting liquid, we need to calculate the heat required for each step separately and then add them together.
Step 1: Heat required to melt ice
The heat required to melt ice (also known as the heat of fusion) can be calculated using the formula:
Q = m × ΔHf
Where:
Q = heat required
m = mass of ice
ΔHf = heat of fusion for ice
The specific heat of fusion for ice is approximately 334 J/g. Thus, the heat required to melt 50.0 g of ice can be calculated as:
Q1 = 50.0 g × 334 J/g
Step 2: Heat required to raise the temperature of the liquid
The heat required to raise the temperature of a substance can be calculated using the formula:
Q = m × C × ΔT
Where:
Q = heat required
m = mass of substance
C = specific heat capacity of substance
ΔT = change in temperature
The specific heat capacity of liquid water is approximately 4.18 J/g°C.
The change in temperature is 65.0°C - 0°C = 65.0°C.
Thus, the heat required to raise the temperature of the liquid can be calculated as:
Q2 = 50.0 g × 4.18 J/g°C × 65.0°C
Finally, to find the total amount of heat required, we add the heat required for each step:
Total heat required = Q1 + Q2
I'll calculate the values for you now.
To calculate the total number of joules needed to melt the ice and warm the resulting liquid, we need to consider two processes:
1. Melting the ice:
The energy required to melt ice at 0°C is given by the formula:
Q = m * ΔHf
where:
- Q is the energy (in joules) required to melt the ice,
- m is the mass of the ice (50.0g in this case), and
- ΔHf is the heat of fusion for ice, which is equal to 334 J/g.
Substituting the given values:
Q = 50.0g * 334J/g
2. Warming the liquid:
The energy required to raise the temperature of the liquid from 0°C to 65°C can be calculated using the formula:
Q = m * C * ΔT
where:
- Q is the energy (in joules) required to heat the liquid,
- m is the mass of the liquid (also 50.0g in this case),
- C is the specific heat capacity of water, which is approximately 4.18 J/g°C, and
- ΔT is the change in temperature, which is 65°C - 0°C = 65°C.
Substituting the given values:
Q = 50.0g * 4.18J/g°C * 65°C
To find the total energy required, we need to sum up the energy required for both processes:
Total-Q = Q-melting + Q-warming
Now, you can calculate the total joules needed by substituting the calculated values into the equation and perform the addition.
1679
q1 to melt ice at zero.
q1 = mass ice x delta H fusion.
q2 to warm water from zero C to 65 C.
q2 = mass water x specific heat water x (Tfinal-Tinitial)
Total q = q1 + q2.