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40.79 H2O kj/moles x 1 moles/18 grams= 2.266/1000=0.002266 joules/grams
Dahlia Kemmer
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∙ 15y agoI am guessing that you actually mean "kilojoules per mole" and "joules per gram", so the question probably ought to read "How do you convert kJ / mol to J / gram?" (I have put in the "divided by" signs). In order to answer the question you need a third piece of information: "grams per mole" or "g / mol". This is sometimes called the molecular weight of the substance, or (better) the "molar mass" of the substance. As an example, the molecular weight of water (H2O) is roughly 18 grams per mole. This is because each Hydrogen atom has a mass of approximately 1 gram per mole, and each Oxygen atom has a mass of approximately 16 grams per mole. 2H + 1O = H2O. So if the number of kilojoules per mole is "X" and the number of grams per mole is "Y" then X kJ/mol ÷ Y g/mol = X/Y kJ/g = 1000X/Y J/gram
Wiki User
∙ 7y agoThe situation is similar as for the regular mole. There cannot be a standard conversion between kg-mole and kg, since they measure very different things. For a specific substance, you need to know the Atomic Mass or the molecular mass of the substance under consideration, and multiply by that number. For example, one kilogram-mole of carbon-12 has 12 kilograms, since the atomic mass of carbon-12 is 12.
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∙ 11y agoThere is no universal conversion, since they really measure different tings. 1 kilojoule, of course is a thousand joule. Now, about the mole and grams... You'll have to know what substance you are talking about, and find out how many grams per mol the substance has. This is equivalent to the substance's molecular mass. If (for example) each molecule has a mass of 100 amu (atomic mass units), that is equivalent to the substance having 100 grams per mole. In this example, you would divide the 6010 joules by 100.
Wiki User
∙ 12y agoGram is a unit of mass where as joule is unit of energy. so we cant convert them.
Wiki User
∙ 13y agoYou multiply it by Avogadro's number, then divide it by 1000.
Wiki User
∙ 10y agoJust divide by one thausand (1000) to convert from J per mole to KJ per mole.
Wiki User
∙ 7y agoKg/mol is the molar mass of a compound expressed in kilograms per mole.
Asteria
40.79KJ/mol change to J/g
Wiki User
∙ 11y agoHKHDYULYJH
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A sample of 1mol of water is condensed isothermally and reversibly to liquid water at 100 degreethe standard enthalpy of vaporization of water is 40.656kj per mole find work and heat?
*H= -(1.00 mol)(40.656kJ/mol) = -40.7 kJ * since q=H (@ constant pressure) there for q= -40.7 kJ *w=nRT =(1.00 mol)(8.315 J/mol.K)(373K) = 3.1 kJ * U= H-nRT = (-40.7kJ)-(1.00 mol)(8.315 J/mol.K)(373K) = -43.8kJ
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 much energy in joules must be absorbed to convert to Na all the atoms present in 1mg of gaseous Na when the first ionization energy is 495.8 kj per mol?
21.6 J
How can you calculate the enthalpy change for combustion of ethane?
The Gibbs free energy change is calculated from the expression Δ G = Δ H - T(Δ S) For the combustion of ethene (assuming it takes place at 25oC): C2H4 + 3O2 --> 2CO2 + 2H2O you need to find the enthalpy and entropy changes, which are Δ H (combustion) = - 1400 kJ/mol Δ S (combustion) = - 1102 J/mol/K Substituting into the first equation, remembering to divide the entropy value by 1000 because it's in J per mol per kelvin, not kJ, and converting the 25 degrees C to kelvin, we get: Δ G = -1314.35 kJ http://www.docbrown.info/page07/delta3SGc.htm
If 6 moles of a compound produce 84 J of energy what is the H reaction in J mol?
-14 J/Mol
A sample of 1mol of water is condensed isothermally and reversibly to liquid water at 100 degreethe standard enthalpy of vaporization of water is 40.656kj per mole find work and heat?
*H= -(1.00 mol)(40.656kJ/mol) = -40.7 kJ * since q=H (@ constant pressure) there for q= -40.7 kJ *w=nRT =(1.00 mol)(8.315 J/mol.K)(373K) = 3.1 kJ * U= H-nRT = (-40.7kJ)-(1.00 mol)(8.315 J/mol.K)(373K) = -43.8kJ
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.
If a reaction has an enthalpy of -54.32 kJ/mol and an entropy of -354.2 J/(K*mol), what is the Gibbs free Energy at 54.3(degrees c)?
DeltaG = DeltaH - TDeltaS dG = -54.32 kJ/mol - (54'32+273)K(-354.2J/molK) NB Thevtemperature is quoted in Kelvin(K) and the Entropy must be converted to kJ by dividing by '1000'/ Hence dG = - 54.32kJ/mol - (327.32K)(-0.3542 kJ/molK) NB The 'K' cancels out. Then maker the multiplication dG = -54/32 kJ/mol - - 115.94 kJ/mol Note the double minus; it becomes plus(+). Hence dG = -54.32kj/mol + 115.94 kJ/mol dG = (+)61.61 kJ/mol Since dG is positive, the reaction is NOT thermodynamically feasible.
What quantity must the heat capacity of an object be divided to obtain the specific heat of that material?
Heat capacity is in the measurement of (kilo)Joules per mol degree Kelvin (J/mol K) Specific heat capacity is in joules/gram degree Kelvin (J/ gram K) Converting between the two is rather simple. To convert to specific heat capacity, divide the molar heat capacity by the molar mass of the molecule in question. eg. ( J/ mol K) / (grams/mol ) = J/ gram K, because mols will cancel.
By what quantity must the heat capacity of an object be divided to obtain the specific heat of that material?
Heat capacity is in the measurement of (kilo)Joules per mol degree Kelvin (J/mol K) Specific heat capacity is in joules/gram degree Kelvin (J/ gram K) Converting between the two is rather simple. To convert to specific heat capacity, divide the molar heat capacity by the molar mass of the molecule in question. eg. ( J/ mol K) / (grams/mol ) = J/ gram K, because mols will cancel.
How much energy in joules must be absorbed to convert to Na all the atoms present in 1mg of gaseous Na when the first ionization energy is 495.8 kj per mol?
21.6 J
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
How do you convert J per mol to J per Photon?
Multiply by avagardoes number
What is the change in energy ΔE in kilojoules per mole of hydrogen atoms for an electron transition from n6 to n2?
The change in energy is -312KJ/mol. E=2.18*10^-18[ (1/2^2)-(1/9^2) ] =5.1884*10^-19 J/atom Divide by 1000 to convert to Kj =5.1884*10^-22KJ/atom 5.1884*10^-22KJ/atom x 6.022*10^23 (avo. #) atoms = -312KJ/Mol 1 Mol
How can you calculate the enthalpy change for combustion of ethane?
The Gibbs free energy change is calculated from the expression Δ G = Δ H - T(Δ S) For the combustion of ethene (assuming it takes place at 25oC): C2H4 + 3O2 --> 2CO2 + 2H2O you need to find the enthalpy and entropy changes, which are Δ H (combustion) = - 1400 kJ/mol Δ S (combustion) = - 1102 J/mol/K Substituting into the first equation, remembering to divide the entropy value by 1000 because it's in J per mol per kelvin, not kJ, and converting the 25 degrees C to kelvin, we get: Δ G = -1314.35 kJ http://www.docbrown.info/page07/delta3SGc.htm
What is the lattice energy of CaCo3?
CaCO3 forms different crystal sructures. Calcite the most common has a latice energy of 2814 KJ/mol. Vaterite 2777 Kj/mol , Anagorite 2820 Kj/mol. reference J Am Chem Soc Vol 122 No.4 2000. from tabulated literature data
How do you use the Gibbs free energy equation to find the Gibbs free energy change for the formation of nitrosyl chloride?
-54.6 kJΔG = (-1218.3) - (298)(-29.9)(1/1000)**apex**-225.3 kjδg = (-905.4) - (298)(180.5)(1/1000)29.54 kJΔG°rxn = (1 mol)(65.27 kJ/mol) + (2 mol)(-33.56 kJ/mol) - (1 mol)(-50.72 kJ/mol) - (4 mol)(238.3 kJ/mol)
