How many calories of heat are necessary to raise the temperature of 200g of ice at -30 degrees celsius to steam at 130 degrees? Show graph and work.
Divide this up into heat regions:
heating the ice from -30 to 0
melting the ice at 0
heating the water from 0 to 100
vaporizing the water at 100
heating the steam from 100 to 130
Add the heats to get total heat.
Calories? I thought calories went out 50 years ago. Joules is pretty standard unit of heat now.
what do you mean by add all the heats. Like add all the numbers you just gave me or what. I don't get it?
calculate the heat to accomplish each of the items listed, then add them up.
To find the number of calories of heat required to raise the temperature of a substance, you can use the equation:
Q = mcΔT
Where:
Q represents the amount of heat energy
m is the mass of the substance in grams
c is the specific heat capacity of the substance
ΔT is the change in temperature
In this case, we need to find the heat required to raise the temperature of 200g of ice from -30 degrees Celsius to steam at 130 degrees Celsius.
First, we need to consider the different stages involved:
1. Heating the ice from -30 degrees Celsius to 0 degrees Celsius - At this stage, the ice absorbs heat without a change in temperature, undergoing a phase change from solid to liquid.
2. Heating the liquid water from 0 degrees Celsius to 100 degrees Celsius - In this stage, the liquid water absorbs heat and its temperature rises.
3. Heating the steam from 100 degrees Celsius to 130 degrees Celsius - At this stage, the steam absorbs heat, causing its temperature to rise further.
To calculate the heat required at each stage, we need to find the specific heat capacity for each phase of water and use the equation mentioned earlier.
Here are the values for specific heat capacity (c) and heat of fusion/vaporization (ΔH) for water:
- Ice: c = 0.5 cal/g°C
- Liquid water: c = 1 cal/g°C
- Steam: c = 0.48 cal/g°C
- Ice to Water:
Q1 = (mass of ice) x (specific heat capacity of ice) x (change in temperature from -30°C to 0°C)
Q1 = 200g x 0.5 cal/g°C x (0 - (-30))°C
Q1 = 200g x 0.5 cal/g°C x 30°C
Q1 = 3000 cal
- Water to Steam:
Q2 = (mass of water) x (specific heat capacity of water) x (change in temperature from 0°C to 100°C)
Q2 = 200g x 1 cal/g°C x (100 - 0)°C
Q2 = 200g x 1 cal/g°C x 100°C
Q2 = 20000 cal
- Steam to 130°C:
Q3 = (mass of steam) x (specific heat capacity of steam) x (change in temperature from 100°C to 130°C)
Q3 = 200g x 0.48 cal/g°C x (130 - 100)°C
Q3 = 200g x 0.48 cal/g°C x 30°C
Q3 = 2880 cal
Finally, to find the total heat required, we add up the values for each stage:
Total heat required = Q1 + Q2 + Q3
Total heat required = 3000 cal + 20000 cal + 2880 cal
Total heat required = 25980 cal
To represent this information graphically, you can create a bar graph that shows the heat required at each stage (Q1, Q2, Q3) and label the stages accordingly: "Ice to Water," "Water to Steam," and "Steam to 130°C". The total heat required (25980 cal) can be shown as the sum of the three bars.
I hope this explanation helps you understand how to calculate the heat required to raise the temperature of ice to steam using specific heat capacities and the equation Q = mcΔT.