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How much energy would it take to melt a 100g sample of copper at its melting point?
You can use this value to estimate the energy required to heat a 100 g of copper by 5 °C, i.e., Q = m x Cp x ΔT = 0.1 * 385 * 5 = 192.5 J.
How much energy does it take to melt?
This energy is termed latent heat since it does not result in a change in the temperature of the water molecules – thermometers cannot measure this energy. A total of 334 J of energy are required to melt 1 g of ice at 0°C, which is called the latent heat of melting.
How many joules does it take to melt 50 grams of ice?
The answer is 153.7kJ .
How much energy does it take to melt silver 100g?
Completion : You will now need to actually do the melting, wich take an amount of energy known as the latent heat of fusion, or enthalpy of fusion. In the case of silver it’s 11.3 kJ/mol, a mol of silver weight 107.87g so if you want 100g you will need (100/107.87)*100 = 92.7mol, wich mean 11.3*0.927 = 10.5kJ.
How do you calculate the melting point of silver?
First you need the specific heat of said material (amount of energy required to heat one kilogram of one degree), wich in the case of silver, is 0.23kj/kg Then you need the melting point of your material, wich in the case of silver, is 961,8 °C.
How do you calculate the heat needed to melt ice?
This means for every mole of ice we melt we must apply 6.02 kj of heat. We can calculate the heat needed with the following equation: #q=nxxDeltaH#. where: #q# = heat. #n# = moles. #DeltaH# = enthalpy. In this problem we would like to calculate the heat needed to melt 35 grams of ice at 0 °C.
How do you calculate the amount of heat required to vaporize?
Use the formula q = m·ΔH v in which q = heat energy, m = mass, and ΔH v = heat of vaporization. The amount of heat required to change 25 grams of water into steam is 56425 joules or 13500 calories.