q = m x C x ΔT
q = amount of heat energy gained or lost in calories
m = mass of substance (in this case water) in grams = 10g
C = heat capacity of substance (in this case water) = 1cal/gram•oC
Tf = final temperature = 32 oC
Ti = initial temperature = 0 oC
ΔT = (Tf - Ti) = 32 oC
q = 10g x 1cal/gram•oC x 32 oC = 320 calories
The heat energy required to melt ice at 0 degrees Celsius is called the heat of fusion. For ice, the heat of fusion is approximately 334 J/g. To convert this to calories, divide by 4.184 J/cal, which gives you approximately 80 calories of heat energy needed to melt 10 grams of ice.
80 calories per gram (called the latent heat of fusion) 80 x 255.67 = 20453.6 calories
For water, the heat of fusion is 80 cal/g. So in other words, this is how many calories are needed to melt 1 gram of water that is frozen. Conversely, when you freeze 1 gram of water, you remove 80 calories of heat from it.... So, you multiply the calories needed to unfreeze a gram of water by the number of grams you have. In this case, 80 * 25 = 2000 Calories
Using the formula Q=mcΔT, the amount of heat energy required is (30g)(4.18J g-1 K-1)(12K) = 1504.8J = 360 calories.
To calculate this, we can use the formula: energy needed = mass * heat of fusion. The heat of fusion for ice is 334 J/g. Thus, the energy needed to melt 5 grams of ice is 5 grams * 334 J/g = 1670 Joules.
The heat energy required to melt ice at 0 degrees Celsius is called the heat of fusion. For ice, the heat of fusion is approximately 334 J/g. To convert this to calories, divide by 4.184 J/cal, which gives you approximately 80 calories of heat energy needed to melt 10 grams of ice.
Specific heat for aluminium = 0.214 Heat required = 38.2 x 0.214 x (275 - 102) = 1414.24 calories
The answer is 2 calories.
how many calories are required to melt a 1.52g ice cube?
To melt 10 grams of ice at 0 degrees Celsius, it would require 80 calories of heat energy per gram, so a total of 800 calories (80 calories/gram * 10 grams = 800 calories) would be needed.
80 calories per gram (called the latent heat of fusion) 80 x 255.67 = 20453.6 calories
Specific heat is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius, while calories are a unit of measurement for energy. Specific heat helps determine how much heat energy is needed to raise the temperature of a substance, while calories measure the amount of energy obtained from food or released during chemical reactions.
To calculate the energy required to heat water, you would need to know the specific heat capacity of water. The specific heat capacity of water is 4.18 J/g°C. Assuming we are heating the water by 1°C, the energy required would be 46.0g * 4.18J/g°C * 1°C = 192.28 Joules.
For water, the heat of fusion is 80 cal/g. So in other words, this is how many calories are needed to melt 1 gram of water that is frozen. Conversely, when you freeze 1 gram of water, you remove 80 calories of heat from it.... So, you multiply the calories needed to unfreeze a gram of water by the number of grams you have. In this case, 80 * 25 = 2000 Calories
Toluene had heat of vaporization of 38.06 kJ/mol Toluene molecular mass is 92.14 g/mol You just need to convert heat of vaporization into kJ/g basis and multiply your 5 gram to get the required amount of heat.
calories.
The needed heat is:Q = 10 x 20 x 0,031 = 6,2 calories