You look up the specific heat of copper (per mass unit). Then you multiply specific heat x mass x temperature difference.
The specific heat capacity of copper is 0.385 J/g°C. To calculate the heat energy required, you use the formula: Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. Plugging the values in, you get Q = 6g * 0.385 J/g°C * (150°C - 100°C) = 92.4 Joules.
To calculate the time taken to raise the temperature by 10 degrees, you would need to know the rate at which the temperature is increasing. This can be determined by dividing the change in temperature (10 degrees) by the rate of temperature increase. The result will give you the time it takes to raise the temperature by 10 degrees.
To calculate the energy released when the copper cools from 1083°C to 25°C, you need to use the formula: Q = mcΔT, where Q is the energy released, m is the mass of the copper, c is the specific heat capacity of copper, and ΔT is the change in temperature. First, find the change in temperature: ΔT = 1083°C - 25°C = 1058°C. Now plug in these values into the formula: Q = 28.9g * 385 J/g°C * 1058°C. Calculate the energy released in Joules.
The amount of heat energy required can be calculated using the formula: Q = mcΔT. Given m = 0.362 kg, c = 390 J/kg°C for copper, and ΔT = (60.0 - 23.0) = 37.0 °C, plug these values into the formula to find the heat energy required to raise the temperature of the copper.
To calculate the energy needed to change ice at -32.9 degrees to water at 75 degrees, you need to consider the energy required for three steps: Heating ice from -32.9 degrees to 0 degrees (specific heat capacity of ice) Melting ice at 0 degrees into water at 0 degrees (latent heat of fusion of ice) Heating water from 0 degrees to 75 degrees (specific heat capacity of water) Once you have the energy needed for each step, you can add them together to find the total energy required.
You cannot. You need the mass of the piece of copper.
The specific heat capacity of copper is 0.385 J/g°C. To calculate the heat energy required, you use the formula: Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. Plugging the values in, you get Q = 6g * 0.385 J/g°C * (150°C - 100°C) = 92.4 Joules.
To calculate the time taken to raise the temperature by 10 degrees, you would need to know the rate at which the temperature is increasing. This can be determined by dividing the change in temperature (10 degrees) by the rate of temperature increase. The result will give you the time it takes to raise the temperature by 10 degrees.
To calculate the energy released when the copper cools from 1083°C to 25°C, you need to use the formula: Q = mcΔT, where Q is the energy released, m is the mass of the copper, c is the specific heat capacity of copper, and ΔT is the change in temperature. First, find the change in temperature: ΔT = 1083°C - 25°C = 1058°C. Now plug in these values into the formula: Q = 28.9g * 385 J/g°C * 1058°C. Calculate the energy released in Joules.
The amount of heat energy required can be calculated using the formula: Q = mcΔT. Given m = 0.362 kg, c = 390 J/kg°C for copper, and ΔT = (60.0 - 23.0) = 37.0 °C, plug these values into the formula to find the heat energy required to raise the temperature of the copper.
O.385x1x2=0.77 Answer: 0.77
I thought I answered this. As I said before, I am too lazy to look up the specific heat of copper (google it ) and I assume the temperature initial is the standard 25 Celsius. Here is the set-up. q(amount of energy in Joules ) = ( 50g Copper)(specific heat of copper in J/gC )(55C-25C)
copper's melting point is 1,083°C and its boiling point is 2,595°C just for fun A coin is usually, made of copper or a copper alloy. But the question was what temperature does it burn at - I'd like to know too - when copper is molten it's surface emits a blue flame, which is presumably burning copper, this happens as soon as it melts.
To calculate the heat energy required, you can use the formula: Q = mcΔT, where Q is the heat energy, m is the mass of the copper (0.365 kg), c is the specific heat capacity of copper (0.0920 J/g°C), and ΔT is the change in temperature (60.0°C - 23.0°C). First, convert the mass to grams and then plug the values into the formula to find the heat energy required.
To calculate the energy needed to change ice at -32.9 degrees to water at 75 degrees, you need to consider the energy required for three steps: Heating ice from -32.9 degrees to 0 degrees (specific heat capacity of ice) Melting ice at 0 degrees into water at 0 degrees (latent heat of fusion of ice) Heating water from 0 degrees to 75 degrees (specific heat capacity of water) Once you have the energy needed for each step, you can add them together to find the total energy required.
To investigate the Fermi energy of copper, you could perform a Hall effect experiment by applying a magnetic field to a copper sample and measuring the Hall voltage. By analyzing the Hall voltage in conjunction with the magnetic field, you can determine the carrier density and then calculate the Fermi energy using the relationship with the Fermi level. Ensure the experiment is conducted at low temperatures to minimize thermal effects.
The amount of energy in hot copper is determined by its temperature and mass. This energy is typically measured in joules (J) or calories (cal). The energy content can be calculated using the specific heat capacity of copper and the change in temperature.