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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 else can I help you with?
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.
How much energy is gained by 3 grams of ice when it changes to water?
The energy needed to change ice into water is called the heat of fusion. For ice, this value is around 334 joules per gram. So, for 3 grams of ice, the energy gained when it changes to water would be around 1002 joules (334 joules/gram * 3 grams).
How much energy is required to raise 21kg of water by 2 degrees Celsius?
The specific heat capacity of water is 4.18 J/g°C. To calculate the energy required to raise 21 kg of water by 2 degrees Celsius, use the formula: Energy = mass x specific heat capacity x temperature change. Plugging in the values, the energy required is 21,084 Joules.
What is the total number of joules required to melt 100 grams of ice at 0 c to liquid water at 0 c?
The total energy required to melt ice at 0°C to liquid water at 0°C is known as the heat of fusion. For water, the heat of fusion is 334 J/g. Therefore, to melt 100 grams of ice, you would need 100 grams * 334 J/g = 33400 Joules of energy.
How much energy is required to raise water temp 1 degree Celsius?
The amount of energy required to raise the temperature of water by 1 degree Celsius is known as its specific heat capacity. For water, the specific heat capacity is 4.18 Joules/gram°C. This means that it takes 4.18 Joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
Specific heat of water equals?
4.18 joules over grams n temp
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.
Which process required water to gain 2260 joules of energy per gram?
The process you are referring to is called water having a specific heat capacity of 4.184 J/g°C. This means that it takes 4.184 joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius. In this case, to gain 2260 joules of energy, it would take approximately 540.3 grams of water.
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 much heat is required to raise the temperature to 5.0 mL of water from 2.50 degrees Celsius to 75 degrees Celsius?
Density = grams/ml 1.00 g/ml = X g/5.0 ml = 5.0 grams water ============== q(joules) = mass * specific heat * change in temp. q = (5.0 grams)(4.180 J/gC)(75 C - 2.50 C) = 1515.25 Joules ---------------------------------/4.184 = 362 calories -------------------
How much energy is gained by 3 grams of ice when it changes to water?
The energy needed to change ice into water is called the heat of fusion. For ice, this value is around 334 joules per gram. So, for 3 grams of ice, the energy gained when it changes to water would be around 1002 joules (334 joules/gram * 3 grams).
How much energy is required to raise 21kg of water by 2 degrees Celsius?
The specific heat capacity of water is 4.18 J/g°C. To calculate the energy required to raise 21 kg of water by 2 degrees Celsius, use the formula: Energy = mass x specific heat capacity x temperature change. Plugging in the values, the energy required is 21,084 Joules.
How many joules of energy are necessary to heat a smaple of water with a mass of 46.0 grams from 0.0 c to 100.0 c?
Water has a specific heat of 4.18J/gC, so set up the specific heat equation: C (spec. heat)=q (joules)/mass x temp. change, so: 4.18 (spec. heat of water) = q/46g(100deg), so q = 4.18(4,600) = 19,228 joules (or 19.228 kJ).
What is the total number of joules required to melt 100 grams of ice at 0 c to liquid water at 0 c?
The total energy required to melt ice at 0°C to liquid water at 0°C is known as the heat of fusion. For water, the heat of fusion is 334 J/g. Therefore, to melt 100 grams of ice, you would need 100 grams * 334 J/g = 33400 Joules of energy.
How much energy is required to raise water temp 1 degree Celsius?
The amount of energy required to raise the temperature of water by 1 degree Celsius is known as its specific heat capacity. For water, the specific heat capacity is 4.18 Joules/gram°C. This means that it takes 4.18 Joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
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
How many joules are needed to melt 2 grams of water?
2,26 Kj are necessary
