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by multiplication by the right cionversion factor.
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The heat of vaporization for liquid zinc is 1.76 kJ per gram. How much heat is needed to boil 11.2 g of liquid zinc already at its boiling point?
Multiply delta H (1.76 kJ/g) by mass (11.2g) That results in 19.7 kJ, convert to J. (1 kJ=1000J) The answer would be 19,700 J or 19.7 kJ, depending on your units.
What is the value for g at 5000 k if h -220 kj mol and s equals -0.05 kj molk?
-18 kj/mol
What is a kj?
KJ means kill joy
How much energy does it take to boil 100 mL of water (Refer to table of constants for water.)?
100 mL × × × 40.65 kJ/mol = 226 kJ
When 100 g of gasoline undergoes combustion 9560 kJ of energy are released Express the heat released 9560 kJ in kilocalories?
1 kJ is approximately 0.239 kcal9560 kJ * (0.239 kcal/kJ) = 2284.84 kcal
How do you get the kJ solar energy in on hour?
convert 9,158,960 km^2 to kJ
How do I convert the latent heat of condensation of water 334 kJkg into a volumetric measurement of kJ m3?
Well 1 kg of water is 1 liter, so 334 kJ/kg would become 334,000 kJ/m3
The heat of vaporization for liquid zinc is 1.76 kJ per gram. How much heat is needed to boil 11.2 g of liquid zinc already at its boiling point?
Multiply delta H (1.76 kJ/g) by mass (11.2g) That results in 19.7 kJ, convert to J. (1 kJ=1000J) The answer would be 19,700 J or 19.7 kJ, depending on your units.
How do you convert kJ-kg-min to kJ-min?
We must assume that this is an exercise in unit analysis. To convert from kilojoule-kilogram-minute to kilojoule-minute requires you to get rid of the kilogram somehow. That means you must divide by kilograms or multiply by kg-1, which is equivalent to 1/kg.
How many calories in 150ml of semi skimmed milk?
between 17 and 20 calories
How many calories burned if burned 400kj?
to convert kj to cal divide by 4.1 therefore: 400/ 4.1 = 97 calories
How many kilojoules should an 11 year old girl eat a day?
To convert food calories to kJ, multiply by 4.184. To convert kJ to food calories, divide by 4.184. For example, a 100 calorie serving of cookies contains 418 kJ. To answer the question it depends on activity level and goals: Active: 2,000 calories (8,368 KJ) Non active, maintain weight: 1800 calories (7,531 KJ) Weight loss: 1500 calories (6,276 KJ) Extreme weight loss: 1000 calories (4,184 KJ)
Calculating ionization energy AP chemistry?
This is my QustionListed below are ionization energies for removing successive electrons from various atoms of the third period. Which of the following lists corresponds to the ionization energies for phosphorus?a. 496 kJ, 4,560 kJ (I.E. for the first two electrons)b. 738 kJ, 1,450 kJ, 7,730 kJ (I.E. for the first three electrons)c. 578 kJ, 1,820 kJ, 2,750 kJ, 11,600 kJ (I.E. for the first four electrons)d. 786 kJ, 1,580 kJ, 3,230 kJ, 4,360 kJ, 16,100 kJ (I.E. for the first five electrons)e. 1,012 kJ, 1,900 kJ, 2,910 kJ, 4,960 kJ, 6,270 kJ (I.E. for the first five electrons)
How much energy must be removed from a 94.4 g sample of benzene at 322.0K to solidify the sample and lower the temp to 205.0 K?
Known info: mass Benzene = 94.4 ΔHfus = 9.8 kj/mol Specific Heat liquid = Cliq = 1.73 J/g Specific Heat Solid = Csolid = 1.51 J/g Temp Melting = 279.0 K 3 Steps A) q = (mass)(Cliq)(ΔT) for change in temp use (322- 279), you're going from the highest temp of 322 K to the point the benzene would melt at 279 K q = (94.4)(1.73)(43) q = 7022.416 convert to kj = 7.022 kj B) use q = (n)( ΔHfus) molar mass = 78.11 convert to moles => 94.4/78.11 = 1.21 q=(1.21)(9.8) q=11.8 kj C) q = (mass)(Csolid)(ΔT) for change in temp here you're going from the melting point to the low temp given. use (279-205) q = (94.4)(1.51)(74) q = 10548.256 convert to kj => 10.548 kj now add all 3 steps together. A + B + C = final answer (7.022 kj) + (11.8 kj) + (10.548 kj) = 29.4 kj
Is there any relationship between the kJ or Kcal of fruit and its ability to produce electricity?
Kj and KCal are units of energy. All energy can be measured in the same units, but that doesn't necessarily mean that you can easily convert the chemical energy in food, to electrical energy.
How do you convert kilojoules to joules?
To convert from kilojoules to joules you have divide by 1000. meaning 1 kilo joule is equal to 1000 joules.
How much heat energy in kilojoules is required to convert 41.0g of ice at -18.0 degrees C to water at 25.0 degrees C?
19.7 kJ
