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How much work did a system do in kJ when a system absorbs 650 J during a change and the value was -2.37?
The work done by the system can be calculated using the formula: Work = Force × Distance × cos(θ). Since work is given as -2.37 kJ, we convert this value to joules (1 kJ = 1000 J). So, the work done is -2.37 kJ × 1000 J/kJ = -2370 J. Therefore, the work done by the system when it absorbs 650 J of energy during a change is -2370 J + 650 J = -1720 J or -1.72 kJ.
Energy in one mole of glucose in joules?
The energy content of one mole of glucose is approximately 2,810 kilojoules (kJ) or 2,810,000 joules (J).
How many kj does 1 gram of protein contain?
One gram of protein contains about 4 kilojoules (kJ) of energy.
How many kj in 1 gram of fat?
There are 9 kilojoules (kJ) in 1 gram of fat.
How many KJ in 1 gram of protein?
There are approximately 17 kilojoules (kJ) in 1 gram of protein.
What is the tango's apparel?
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How much work did a system do in kJ when a system absorbs 650 J during a change and the value was -2.37?
The work done by the system can be calculated using the formula: Work = Force × Distance × cos(θ). Since work is given as -2.37 kJ, we convert this value to joules (1 kJ = 1000 J). So, the work done is -2.37 kJ × 1000 J/kJ = -2370 J. Therefore, the work done by the system when it absorbs 650 J of energy during a change is -2370 J + 650 J = -1720 J or -1.72 kJ.
What is 3923.7552 J into Kj?
To convert joules to kilojoules, divide by 1000. Therefore, 3923.7552 J is equal to 3.9238 kJ.
Energy in one mole of glucose in joules?
The energy content of one mole of glucose is approximately 2,810 kilojoules (kJ) or 2,810,000 joules (J).
If the heat of vaporization for water is 2260 Jg how many kilojoules are required to convert 5.00 g of liquid water at 100C to steam at 100C?
The heat required to vaporize 5.00 g of water is given by: 2260 J/g * 5.00 g = 11300 J. Converting this to kJ gives 11.3 kJ.
How much heat must be added to raise the temp of .4 kg of water from 20 C to 25 C?
Using the specific heat of water as 4180 J/kg/deg, and q = mC∆T one can calculate the heat needed.q = (0.4 kg)(4180 J/kg/deg)(5 deg) = 8360 J = 8.4 kJ (or 8 kJ to one significant figure)
How many kilojoules in one peanut?
3.84 KJ
The initial temperature of 0.8 kg of ice was -5 Celsius. How much energy is needed to cause the ice to start to melt?
specific heat of ice = 2.09 J/g/degree2.09 J/g/deg x 800 g x 5 deg = 8360 J = 8.4 kJ∆Hfusion = 334 J/g0.8kg x 334 J/g x 1000 g/kg x 1 kJ/1000 J = 267 kJ8.4 kJ + 267 kJ = 275.4 kJ
How do you mention kilojoule units?
kJ for kilojoules and J for joules.
How many children does Florence Griffith Joyner have?
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If 3 moles of a compound use 12 J of energy in a reaction what is the H reaction in kJmol?
12 J/3 moles = 4 J/mole. Thus, H of reaction in kJ/mole = 0.004 kJ/mole
What was life like for an average person in france?
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