To convert joules to kilojoules, divide by 1000. Therefore, 3923.7552 J is equal to 3.9238 kJ.
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
To determine the mass of ice that can be melted by 2.0 kJ of energy, we use the latent heat of fusion for ice, which is approximately 334 J/g. First, convert 2.0 kJ to joules (2.0 kJ = 2000 J). Then, divide the total energy by the latent heat: ( \frac{2000 , \text{J}}{334 , \text{J/g}} \approx 5.99 , \text{g} ). Thus, about 6 grams of ice can be melted by 2.0 kJ of energy.
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.
The ∆Hfusion for water is 333.55 J/g. Thus, q = 98.5 g x 333.55 J/g = 32,855 J = 32.9 kJ (3 sig figs)
To determine the mass of water that must form to produce 975 kJ of energy, we can use the concept of the heat of vaporization of water, which is approximately 2260 J/g. First, convert 975 kJ to joules: 975 kJ = 975,000 J. Then, divide the total energy by the heat of vaporization: ( \text{mass} = \frac{975,000 \text{ J}}{2260 \text{ J/g}} \approx 431.87 \text{ g} ). Thus, about 432 grams of water must form to produce 975 kJ of energy.
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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.
The energy E in joules (J) is equal to 1 kilojoule times 1000: E (J) = 1kJ × 1000 = 1000J . So 1 kilojoule (kJ) is equal to 1000 joules (J): 1 kJ = 1000 J .
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
To determine the mass of ice that can be melted by 2.0 kJ of energy, we use the latent heat of fusion for ice, which is approximately 334 J/g. First, convert 2.0 kJ to joules (2.0 kJ = 2000 J). Then, divide the total energy by the latent heat: ( \frac{2000 , \text{J}}{334 , \text{J/g}} \approx 5.99 , \text{g} ). Thus, about 6 grams of ice can be melted by 2.0 kJ of energy.
kJ for kilojoules and J for joules.
12 J/3 moles = 4 J/mole. Thus, H of reaction in kJ/mole = 0.004 kJ/mole
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It is 1000 J. K meand time 10^3
That is an abbreviation for a kilojoules, a metric measure of energy.
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.
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