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How much energy is required to raise the temperature of one liter of water 1 degree centigrade?
The specific heat of water is 4.179 Joules per gram per degree Centigrade. The density of water is 1 gram per cubic centimeter, so one liter is 1000 grams. This means it takes 4179 Joules to raise one liter one degree Centigrade.
How much energy required to heat 100 liters of 30 degree centigrade water to raise 135 degree centigrade?
4186 Joules per liter per deg C. Not clear if we are raising the temperature BY 135 deg or TO 135 deg. So the answer is 4186 x 100 x rise in temperature. (Joules).
What is the relationshio between specific heat and temperature?
The unit of specific heat is Joules per gram per degree (C) or Joules per gram per degree (K). It comes from Q (heat) per mass per change in temperature (T) or Specific heat = Heat (Q)/ Mass(M) . Change in Temperature (Delta T).
By what quantity must the heat capacity of an object be divided to obtain the specific heat of that material?
Heat capacity is in the measurement of (kilo)Joules per mol degree Kelvin (J/mol K) Specific heat capacity is in joules/gram degree Kelvin (J/ gram K) Converting between the two is rather simple. To convert to specific heat capacity, divide the molar heat capacity by the molar mass of the molecule in question. eg. ( J/ mol K) / (grams/mol ) = J/ gram K, because mols will cancel.
What dose a high specific heat tell about a substance?
A high specific heat tells you that it is hard to change the temperature of a substance.
How much energy is required to raise the temperature of one liter of water 1 degree centigrade?
The specific heat of water is 4.179 Joules per gram per degree Centigrade. The density of water is 1 gram per cubic centimeter, so one liter is 1000 grams. This means it takes 4179 Joules to raise one liter one degree Centigrade.
How much energy must be supplied to turn 1 gram of water at 100 degrees centigrade to steam at 100 degree centigrade?
Heat of vaporization of water is 2.26 x 106 joules per kg. Therefore 1 gram of water will need 2.26 x 103 joules.
Specific heat capacity of water?
The specific heat of water is 4.184 J/g*°C, which is read 4.184 Joules per gram degree Celsius. It can also be stated as 1.00 cal/g*°C, which is read calories per gram degree Celsius (same as centigrade). These values mean that it takes 4.184 Joules of energy to raise the temperature of 1 gram of water 1 degree Celsius. Or it takes 1.00 calories of energy to raise the temperature of 1 gram of water 1 degree Celsius. 4.184 Joules = 1.00 calorie
How much energy required to heat 100 liters of 30 degree centigrade water to raise 135 degree centigrade?
4186 Joules per liter per deg C. Not clear if we are raising the temperature BY 135 deg or TO 135 deg. So the answer is 4186 x 100 x rise in temperature. (Joules).
What is correct 4.184 or 4.1868 joules per gram for every change in temperature 1 degree centigrade specific heat of water?
In the steam table and thermochemical variations in the related link below. It may depend on which variation your meaning.
What is the relationshio between specific heat and temperature?
The unit of specific heat is Joules per gram per degree (C) or Joules per gram per degree (K). It comes from Q (heat) per mass per change in temperature (T) or Specific heat = Heat (Q)/ Mass(M) . Change in Temperature (Delta T).
How hot is a joule?
The mechanical equivalent of heat is 4.2 Joules per calorie, so 4.2 Joules can heat 1 gram of water by 1 degree C.
If you wish to heat water from thirty degrees to one hundred degrees how much heat will be required?
70 calories per gram. (The specific heat capacity of water is 1 calorie per gram per degree C.) This could be converted into Joules if necessary using the conversion factor of 1 calorie = 4.18400 Joules.
How do I convert the enthalpy of vaporization of water in joules per gram from kiloJoules per mole?
Lets say, for example the enthalpy is equal to 1200 joules/gram. You take 1200 joules/gram * (# of grams)/one mole [now you can cancel grams and it is now joules/mole.] Then convert the answer to kilojoules by dividing by 1000.
How can things have the same temperatures but different heats?
Two things can have the same temperature but different heats if they have different specific heats. For example, water has a specific heat of 1 joule per gram per degree. Iron has a specific heat of 0.45 joules per gram per degree. So, if you had 1 gram of water and 1 gram of iron, both at 25º, and you added 1 joule of energy, the temperature of water would go up 1 degree to 26º, but the temperature of iron would go up 2.2 degrees to 27.2º.
How many kilojoules in 1 gram of water?
It depends on the temperature of the water. 1 calorie equals roughly 4.184 joules, and 1 calorie equals roughly 1 degree C in a gram of water. (the actual definition includes a specific temperature, I think about 3 degrees C). So you could say that 1 gram of water contains roughly 4.18400 joules per degree above absolute zero, so 1 gram of near-freezing water is about 273 degrees * 4.184 joules/degree = about 1142 joules.
By what quantity must the heat capacity of an object be divided to obtain the specific heat of that material?
Heat capacity is in the measurement of (kilo)Joules per mol degree Kelvin (J/mol K) Specific heat capacity is in joules/gram degree Kelvin (J/ gram K) Converting between the two is rather simple. To convert to specific heat capacity, divide the molar heat capacity by the molar mass of the molecule in question. eg. ( J/ mol K) / (grams/mol ) = J/ gram K, because mols will cancel.
