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What is the total number of joules required to melt 100 grams of ice at 0 c to liquid water at 0 c?
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∙ 12y ago
226,ooo j
Wiki User
∙ 12y ago
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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?
0.131 joules/gram'C x 1.3 grams x (46-25)'C = 3.5763 joules
The specific heat of water is 4.2 joules over g C if you wish to heat 300 grams of water from 30 C to 100 C how much heat will be required?
To solve this you would use the equation q=mCs deltaT, in which q is the amount of energy needed for the reaction (in Joules), m is the mass of the substance in grams, Cs is the specific heat, and deltaT is the change in temperature of the reaction. In this case, q = what you are looking for Cs = 4.184J/g*C m = 46.0 grams delta T = 100.0 degrees celsius q = 46.0g x 4.184j/g*c x 100.0 *c q = 19246.4 Joules
What amount of heat energy is required to raise the temperature of 45 pounds of lead from 62 degrees to 100 degreesF?
Specific heat of lead = 0.160 J/gC 45 pounds (454 grams/ 1 pound) = 20430 grams Use. q(Joules) = mass * specific heat * change in temp. q = (20430 grams)(0.160 J/gC)(100 C - 62 C) = 1.2 X 10^5 Joules ------------------------- or ------------------------- 1.2 X 10^5 Joules (1 calorie/4.184 Joules) = 29688 calories
The temperature of 15 grams of water is increased by 3.0 Celsius degrees How much heat in Joules was absorbed by the water?
I assume you mean 30o Celsius. Use this formula.q(joules) = mass * specific heat * change in temperatureq = (15 grams water)(4.180 J/gC)(40o C - 30o C)= 627 joules==========( perhaps 630 joules to be in significant figures territory )
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams for 0.0?
46 calories (or 192, 464 joules) for each Celsius degree.
What is the total number of joules required to melt 100 grams of ice at 0 C to liquid water at C?
226,ooo j
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
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?
0.131 joules/gram'C x 1.3 grams x (46-25)'C = 3.5763 joules
When 20 grams of water is cooled from 20 C to 10 C the number of joules of heat released is?
200 calories, or approx. 47.84 joules
How many grams is equals 1 joules?
0000000000000000.11 joules
What amount of total heat required to vaporise and then condense liquid?
5 grams of protien
The specific heat of water is 4.2 joules over g C if you wish to heat 300 grams of water from 30 C to 100 C how much heat will be required?
To solve this you would use the equation q=mCs deltaT, in which q is the amount of energy needed for the reaction (in Joules), m is the mass of the substance in grams, Cs is the specific heat, and deltaT is the change in temperature of the reaction. In this case, q = what you are looking for Cs = 4.184J/g*C m = 46.0 grams delta T = 100.0 degrees celsius q = 46.0g x 4.184j/g*c x 100.0 *c q = 19246.4 Joules
How many calories are required to raise the temperature of 150 g sample of gold from 25 Celsius to 175 Celsius?
I will use this formula, the convert. q( in Joules ) = mass * specific heat Au * change in temp. q = nCT q = (150 grams)(0.129 J/gC)(175 C - 25 C) = 2902.5 Joules Now, 1 calorie = 4.184 Joules 2902.5 Joules (1 calorie/4.184 Joules) 694 calories required
How many joules are in 1500 grams?
Voltage is electrical pressure and Joules is a power rating so other info is needed
How many grams equals one liquid ounce?
A liquid (or fluid) ounce is a measure of volume. A gram is a measure of mass. Therefore, the number of grams per fluid ounce of a liquid depends on what the liquid is, specifically on what its density is.
How many joules of heat are requied to melt 40 g of ice at 0 C?
In order to answer this question, you need the enthalpy of fusion of ice, which is 333.55 J/g (Joules/gram). The enthalpy of fusion is the amount of heat that must be absorbed or lost in order to change physical state. The number of Joules required to melt the ice = enthalpy of fusion of ice x mass of ice. Joules needed to melt the ice = 333.55 J/g x 40 g = 13342 J
How do you Convert 40.79 kilojoules per mole to joules per grams?
40.79 H2O kj/moles x 1 moles/18 grams= 2.266/1000=0.002266 joules/grams
