calculate the amount of heat needed to melt 35.0kg of ice at 0*c
To calculate the amount of heat needed to melt a solid substance, we use the formula:
Q = m * ΔHf
where:
Q is the heat energy required (in Joules),
m is the mass of the substance (in kilograms),
and ΔHf is the heat of fusion (specific latent heat) for the substance (in Joules per kilogram).
Given:
m = 35.0 kg (mass of ice)
ΔHf = 334,000 J/kg (heat of fusion for ice)
Now, substitute the given values into the formula:
Q = 35.0 kg * 334,000 J/kg
Q = 11,690,000 J
Therefore, the amount of heat needed to melt 35.0 kg of ice at 0°C is 11,690,000 Joules.
To calculate the amount of heat needed to melt 35.0 kg of ice at 0°C, we need to use the specific heat capacity and latent heat of fusion of ice.
The specific heat capacity of ice is 2.09 J/g°C, which means it takes 2.09 Joules of energy to raise the temperature of 1 gram of ice by 1 degree Celsius.
The latent heat of fusion of ice is 334 J/g, which means it takes 334 Joules of energy to convert 1 gram of ice at 0°C into 1 gram of liquid water at 0°C.
Step 1: Calculate the heat required to raise the temperature of the ice from -273°C to 0°C.
Q1 = mass × specific heat × temperature change
Q1 = 35.0 kg × 2.09 J/g°C × (0 - (-273)°C)
Note: Remember to convert the mass from kg to grams (1 kg = 1000 g).
Q1 = 35,000 g × 2.09 J/g°C × 273°C
Step 2: Calculate the heat required to melt the ice at 0°C.
Q2 = mass × latent heat of fusion
Q2 = 35,000 g × 334 J/g
Step 3: Calculate the total heat required.
Total heat = Q1 + Q2
Finally, sum up Q1 and Q2 to find the total amount of heat required to melt 35.0 kg of ice at 0°C.
To calculate the amount of heat needed to melt a certain amount of ice, you need to use the equation:
Q = m * Hf
where:
Q = amount of heat needed (in joules)
m = mass of the ice (in kilograms)
Hf = heat of fusion for ice (in joules per kilogram)
The heat of fusion for ice is the amount of heat energy required to change 1 kilogram of ice at 0°C to 1 kilogram of water at 0°C, which is approximately 334,000 joules per kilogram.
Now let's plug in the values into the equation:
m = 35.0 kg (given mass of the ice)
Hf = 334,000 J/kg (heat of fusion for ice)
Q = 35.0 kg * 334,000 J/kg
Q ≈ 11,690,000 joules
Therefore, approximately 11,690,000 joules of heat energy is needed to melt 35.0 kg of ice at 0°C.