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How much heat is required to change 0.2kg of ice at -5 degrees to water at 5 degrees?
Heat required for this transition is given as the the sum of three heatsheat required for heating the ice from -5 degree Celsius +latent heat(conversion of ice at zero degree to water at zero degrees)+heat required to heat the water from 0 to 5 degree CelsiusHeating of ice=m x s x delta T,where m is the mass ,s is the specific heat of ice=200x0.5x5=500calmelting of ice=mxlatent heat=200x80=16,000calHeating of water=m x s x delta T,where m is the mass ,s is the specific heat of water =200x1x5=1000calTotal heat required=500+16,000+1000=17,500 cal
How much heat is required to convert 0.3 kilogram of ice to 0 degree celsius at the same temperature?
question makes no sense.....
How much heat is required to convert 1.00 kg of water at 100 degrees Celsius to steam at 100 degrees Celsius?
Assuming standard atmospheric pressure, 2260 kilojoules.
How much natural gas required to heat 1 gallon of water to 140 F?
That completely depends on the temperature of the water when the gas flame is first ignited, which you've neglected to mention.
How much heat energy will be required to lower the temperature of 2.67kg of steam from 282 degrees Celsius to 105 degrees Celsius?
You mean how much heat energy will be lost/transferred as you are losing Joules here. All in steam, so a simple q problem and no change of state. 2.67 kg = 2670 grams q = (2670 grams steam)(2.0 J/gC)(105 C - 282 C) = - 9.45 X 105 Joules ----------------------------------- This much heat energy must be lost to lower the temperature of the steam.
How much does the gt bump bmx bike weigh?
28lbs
How much does Jen Arnold from TLC's the Little Couple weigh?
28lbs, about as much as my 10 month old son.
What is the measurement of how much heat energy is required for a substance to melt?
The measurement of how much heat energy is required for a substance to melt is called the heat of fusion. It is the amount of energy required to change a substance from a solid to a liquid at its melting point.
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 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.
Is the amount of heat required to boil 1kg of water equal to the amount of heat required to melt 1kg of ice?
No, the amount of heat required to boil 1kg of water is much higher than the amount of heat required to melt 1kg of ice. Boiling water requires additional heat to overcome the latent heat of vaporization, while melting ice only requires heat to overcome the latent heat of fusion.
How much heat is required to convert 1 kg of ice to liquid?
lf = 3.35 x 105 J kg-1 This much amount of heat required to convert 1 kg of ice to liquid Mani.Ra
How much heat is required to pyrolyse plastic?
The values are different for each type of plastic.
How much heat is required to convert 0.3 of ice at 0 to water at the same temperature?
The heat required to convert ice at 0°C to water at 0°C is known as the latent heat of fusion. For water, this value is 334 J/g. Therefore, to convert 0.3 g of ice to water at the same temperature, the heat required is 0.3 g * 334 J/g = 100.2 Joules.
If 30.86g of H2O is frozen (from liquid to solid) how much heat energy is required?
No heat (energy) is required to freeze water (from liquid to solid). Freezing RELEASES energy (heat), as it is an exothermic event. If you want to know how much energy is release, you need to know the heat of fusion for water, and then multiply that by the mass of water being frozen.
How much heat energy is required to raise the temperature of 0.365 of copper from 23.0 to 60.0 The specific heat of copper is 0.0920?
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.
How much heat is required to raise the temperature of 0.25 kg of water from 20 Celsius to 30 Celsius?
The specific heat capacity of water is 4186 J/kg*C. To calculate the heat required, use the formula: heat = mass * specific heat capacity * change in temperature. Plugging in the values, the heat required to raise the temperature of 0.25 kg of water by 10 degrees Celsius is approximately 1046.5 Joules.
