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How much heat is required to change kg of ice at C to water at C C?
To change 1 kg of ice at 0°C to water at 0°C, you would need 334 kJ of heat energy. This includes the heat required to raise the temperature of the ice to 0°C (latent heat of fusion) and then to melt it into water at 0°C.
How much heat is requireto raise the temperatureof 5kilogramsof water by 1 kelvin?
The specific heat capacity of water is 4.184 J/g°C. To raise the temperature of 5 kg of water by 1 K, you would need to calculate the total heat energy using the formula Q = m * c * ΔT, where Q is the heat energy, m is the mass of water, c is the specific heat capacity of water, and ΔT is the temperature change.
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.
What is the mount of heat released when 50.0 grams of steam at 100 degrees hits the skin condenses to water at 100 degrees and cool to a body temperature of 37 degrees?
To calculate the heat released, you need to consider three steps: 1. Heat released during condensation of steam to water at 100°C. 2. Heat released as the water cools from 100°C to 37°C. 3. Heat released as the water reaches body temperature at 37°C. The specific heat capacity of water is 4.18 J/g°C and the heat of vaporization for water is 2260 J/g. You need to use the formula: Q = m * c * ΔT or Q = m * L, where Q is the heat released, m is the mass, c is the specific heat capacity, ΔT is the temperature change, and L is the heat of vaporization.
How much heat does it take to warm 21.0g of pure water from 90.0C to 100.0C?
To calculate the heat required to warm the water, you need to use the formula Q = mcΔT, where Q is the heat, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature. First, you need to calculate the temperature change (ΔT = 100.0°C - 90.0°C = 10.0°C). The specific heat capacity of water is 4.184 J/g°C. Plugging these values into the formula gives you: Q = 21.0g * 4.184 J/g°C * 10.0°C. Calculate to find the heat required.
How much heat is required to change kg of ice at C to water at C C?
To change 1 kg of ice at 0°C to water at 0°C, you would need 334 kJ of heat energy. This includes the heat required to raise the temperature of the ice to 0°C (latent heat of fusion) and then to melt it into water at 0°C.
How much heat is requireto raise the temperatureof 5kilogramsof water by 1 kelvin?
The specific heat capacity of water is 4.184 J/g°C. To raise the temperature of 5 kg of water by 1 K, you would need to calculate the total heat energy using the formula Q = m * c * ΔT, where Q is the heat energy, m is the mass of water, c is the specific heat capacity of water, and ΔT is the temperature change.
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.
What is the mount of heat released when 50.0 grams of steam at 100 degrees hits the skin condenses to water at 100 degrees and cool to a body temperature of 37 degrees?
To calculate the heat released, you need to consider three steps: 1. Heat released during condensation of steam to water at 100°C. 2. Heat released as the water cools from 100°C to 37°C. 3. Heat released as the water reaches body temperature at 37°C. The specific heat capacity of water is 4.18 J/g°C and the heat of vaporization for water is 2260 J/g. You need to use the formula: Q = m * c * ΔT or Q = m * L, where Q is the heat released, m is the mass, c is the specific heat capacity, ΔT is the temperature change, and L is the heat of vaporization.
How much heat does it take to warm 21.0g of pure water from 90.0C to 100.0C?
To calculate the heat required to warm the water, you need to use the formula Q = mcΔT, where Q is the heat, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature. First, you need to calculate the temperature change (ΔT = 100.0°C - 90.0°C = 10.0°C). The specific heat capacity of water is 4.184 J/g°C. Plugging these values into the formula gives you: Q = 21.0g * 4.184 J/g°C * 10.0°C. Calculate to find the heat required.
What is the heat content of a gallon of water at a certain temperature?
The heat content of a gallon of water at a certain temperature can be calculated using the specific heat capacity of water (1 calorie/gram °C). For example, to calculate the heat content of a gallon of water at 20°C, you would need to know the mass of the water and apply the formula: heat content = mass of water x specific heat capacity x temperature change.
Write the expression and value for the specific heat of water?
The expression for specific heat is Q = mc(delta T) where Q is the heat added, c is the specific heat, m is the mass, and delta T is the change in temperature in degrees C. Specific heat is the amount of heat per unit of mass needed to raise the temperature by 1 degree C. The specific heat of water is 1 cal/gram degree C = 4.186 joule/gram degree C. Water has a higher specific heat than most common substances.
How many calories does it take to heat 1 liter of water 1 degree?
It takes 1000 calories to heat 1 litre of water 1 degree C.
What is the amount of heat needed to raise the temperature of 1 g of water?
It depends on what your INITIAL and FINAL temperatures are. Assuming you had water at 20°C and wanted to raise it to 50°C You can use the formula: Q = mcΔT Q = Amount of Heat (Energy) m (mass)= 1g c (specific heat capacity) = 4.186J/g°C ΔT = Final Temperature - Initial Temperature = 50°C - 20°C = 30°C Q = 1g x 4.186J/g°C x 30°C Q = 125.58J
How much heat is needed to change 40.0 g of ice at -15.0 degrees c to water at 0.0 degrees c?
To calculate the heat needed, you would first need to raise the temperature of the ice from -15.0°C to 0.0°C, which requires heat. Next, you would need to add heat to melt the ice into water at 0.0°C. The specific heat capacity and heat of fusion of ice would be used in these calculations.
How much heat can be stored in one cubic meter of water in a heat exchanger at 25 C?
Heat stored is based on a change in temperature. If you heat the water to 75 C, then you can extract that heat when the water is cooled to 25 C again. 1 cubic meter of water is 1,000,000 grams Heat absorbed or released = specific heat capacity x mass x change in temperature. = (1 cal / g C) x (1,000,000 g) x (75 - 25)C = 50,000,000 calories lower temperature change means less heat stored.
How much heat in joules would you need to raise the temperature of 1kg of water by 5 and degC?
You would need 20,920 Joules of heat to raise the temperature of 1kg of water by 5°C. This value is calculated using the specific heat capacity of water, which is 4186 J/kg°C.
