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How much heat energy is needed to raise the temperature of a 055kg sample of aluminum from 22.4 degrees celsius to 94.6 degrees celsius?
The heat energy required can be calculated using the formula: Q = mcΔT, where Q is the heat energy, m is the mass of the aluminum (0.055 kg), c is the specific heat capacity of aluminum (900 J/kg°C), and ΔT is the change in temperature (94.6°C - 22.4°C = 72.2°C). Plugging in the values, we get Q = 0.055 kg * 900 J/kg°C * 72.2°C = 3582.7 J. Hence, 3582.7 Joules of heat energy is needed to raise the temperature of the aluminum sample.
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams for 0.0?
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.
The specific heat of gold is 0.131 Joules per gram. Celsius How much energy is required to heat 1.3 grams of gold from 25 Celsius to 46 Celsius?
The change in temperature is 21 degrees Celsius. To calculate the energy required, we use the formula: Energy = mass * specific heat * change in temperature. Plugging in the values, Energy = 1.3g * 0.131 J/g°C * 21°C = 35.247 Joules. Therefore, 35.247 Joules of energy is required to heat 1.3 grams of gold from 25°C to 46°C.
How much energy is required to raise the temperature of 0.2kg of aluminum for 15 degrees celsius to 18 degrees celsius?
The specific heat capacity of aluminum is 0.9 J/g°C. To calculate the energy required to raise the temperature of 0.2kg of aluminum by 3 degrees Celsius, you would use the formula: Energy = mass x specific heat capacity x temperature change. Substituting the values into the formula, Energy = 0.2kg x 0.9 J/g°C x 3°C = 0.54 Joules.
How much heat is required to raise the temperature of a 30.0 g block of aluminum from 25.0ºC to 75.0ºC?
The specific heat capacity of aluminum is 0.897 J/g°C. The heat required can be calculated using 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 in the values, you can calculate how much heat is required.
How much eat in calories is required to heat a 43 g sample of aluminum from 72 F to 145F?
How much heat (in calories) is required to heat a 43 g sample of aluminum from 72 F to 145F
How many joules would be required to heat 0.5kg of aluminum?
The specific heat capacity of aluminum is 0.897 J/g°C. To calculate the energy required to heat 0.5kg of aluminum by a certain temperature change, you would use the formula: Energy = mass x specific heat capacity x temperature change If you have the temperature change, you can plug the values into the formula to find the total energy in joules.
How much heat is required to raise the temp of 106g of aluminum from 96 degree celsius to 121 degree celsius?
Specific heat of aluminum is 0.902 J/gC Use this formula. q(Joules) = mass * specific heat * change in temperature q = 106 grams Al * 0.902 J/gC *(121 C = 96 C) = 2390 Joules of heat
Suppose you want to heat 40g of water by 20c how many joules of heat are required?
334.8 Joules
How much heat in joules to heat a 40 g sample of aluminum from 73 degrees f to 142 degrees f?
q( in Joules ) = mass * specific heat * change in temperature [ convert temps--Tf = Tc(1.80) + 32 ] q = (40 g)(0.90 J/gC)(61.1o C - 22.8o C) = 1.4 X 103 Joules =============
How much heat energy is needed to raise the temperature of a 055kg sample of aluminum from 22.4 degrees celsius to 94.6 degrees celsius?
The heat energy required can be calculated using the formula: Q = mcΔT, where Q is the heat energy, m is the mass of the aluminum (0.055 kg), c is the specific heat capacity of aluminum (900 J/kg°C), and ΔT is the change in temperature (94.6°C - 22.4°C = 72.2°C). Plugging in the values, we get Q = 0.055 kg * 900 J/kg°C * 72.2°C = 3582.7 J. Hence, 3582.7 Joules of heat energy is needed to raise the temperature of the aluminum sample.
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams from 0.0 celsius to 100.0?
419.1 Joules are required to heat one gram of liquid water from 0.01 degC to 100 deg C. So the answer is 419.1*46 = 19278.6
How much energy is required to vaporize 1.5 kg of aluminum (refer to table of latent heat values.)?
To calculate the energy required to vaporize 1.5 kg of aluminum, we need to use the latent heat of vaporization for aluminum, which is approximately 10,900 J/kg. The energy required can be calculated using the formula: Energy = mass × latent heat of vaporization. Thus, for 1.5 kg of aluminum: Energy = 1.5 kg × 10,900 J/kg = 16,350 J. Therefore, 16,350 joules of energy is required to vaporize 1.5 kg of aluminum.
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams for 0.0?
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.
How many joules of heat would be requiredto heat 0.5 kg of aluminum by 2k?
you need to know the specific heat capacity of aluminum first which can be denoted as 'c'. then using the formula: H=MC(dt) where 'dt; is the change in temperature, M is the mass and H is energy needed, you can thus calculate H. i think the value of 'c' for aluminum is around 0.88Jg/K Replace given values in the equation, you will surely get the answer!
How many joules are necessary to heat a sample of water with a mass of 46.0 grams from 0.0?
46 calories (or 192, 464 joules) for each Celsius degree.
How many kilocalories are required to melt 16g of ice?
This heat is 32,48 joules.
