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How much energy is required to raise the temperature of 10.0 grams of granite from 20C to 50C?
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Which has more density 20 grams of granite or cotton balls?
Granite.
How much energy is gained by 3 grams of ice when it changes to water?
No energy is gained. On the contrary, energy is required to make ice melt.
What amount of heat is required to raise the temperature of 350 grams of copper to cause a 25C change?
69
How much energy is needed to increase the temperature of 755 grams of ironfrom 283Kelvin to 403Kelvin?
quite abit
How much energy is needed to raise the temperature of 2.0 grams of water of 5.0 Celsius?
42 J
How much energy is required to raise the temperature of 2kg of iron from 20 C to 23 C?
(Explanation): remember to convert the 2kg to grams, then multiply in this equation Q=(2000)(0.45)(3) to get Q=2700J
What is the specific heat of an unknown substance if 2000J of energy are required to raise the temperature of 4 grams of the substance 5 degrees celsius?
Just use the definition of specific heat. Use the following formula: (energy) = (mass) x (temperature difference) x (specific heat) Replace the amounts you know, and solve for the one you don't - in this case, the specific heat.
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 energy is required to raise 21kg of water by 2 degrees Celsius?
21 Kg = 2100 grams to rise the temperature of this amount of water by 2 degrees Celsius you need 2*2100 = 4200 calories or 17572.8 Joules.
If 150 grams of water changes temperature by 7.2 C how much heat energy flows?
35 kg
When 418 joules of heat energy are added to 10 grams of water at 20C the final temperature of the water will be?
21
What is Water absorption coefficient formula?
If the water is not already at boiling temperature, then you will need equations 1 and 2. If the water is already at boiling temperature, you will only need equation 2.1. Q = m X C X ΔTThis equation is used to calculate how much energy is required to change the temperature of a given object, of given mass, by a given number of degrees.Q = the total amount of energy required, in joulesm = mass, in grams, of the object being heated (in this case, the water)C = the specific heat of the object (for water, 4.186)ΔT = the total change in temperature2. Q = 2.257 joules X mThe 2.257 in this equation is the heat of vaporization of water: that is, the amount of energy, required per gram of water, to boil water: 2.257 joules per gram. If you were using this equation for a different substance, you would have to look up its heat of vaporization, and substitute it in this equation.Q = the amount of energy required, in joulesm = mass, in grams, of the waterFor example, suppose you were asked to calculate how much energy it would take to boil 256 grams of water which is currently at 40 degrees Celsius. We know that the boiling temperature of water is 100 degrees Celsius; therefore the change in temperature, ΔT, is 100 - 40, which equals 60. Calculate as follows:Q = 256 grams X 4.186 X 60°CQ = 64296.96 joulesThis is how much energy it will take to raise the temperature of the water from 40°C to 100°C. Now calculate how much energy it will take to boil the water once it reaches 100°C:Q = 2.257 joules X 256 gramsQ = 577.792 joulesWe now take the energy required to raise the temperature of the water from 40°C to 100°C and add it to the energy required to boil the water:64296.96 joules + 577.792 joules = 64874.752 joulesConvert to kilojoules:64875.752 joules / 1000 = 64.875752 kilojoulesRound to 64.88 kilojoules.If you are required to express your answer in scientific notation, then express it as6.488 x 103 kilojoules.
