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40.79 H2O kj/moles x 1 moles/18 grams= 2.266/1000=0.002266 joules/grams
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What is the heat of solution for barium chloride in joules?
The heat of solution for barium chloride is -61.7 kJ/mol. To convert this to joules, multiply by 1000 to get -61,700 J/mol.
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?
The first step is to calculate how many moles of Na are present in 1 mg (0.001 g) of Na. Since the molar mass of Na is 22.98977 g/mol, there are 0.000043 moles of Na. Next, convert the ionization energy to joules by multiplying by 1000 (1 kJ = 1000 J) to get 495,800 J/mol. Finally, multiply the number of moles by the energy per mole to find the total energy required: 495,800 J/mol * 0.000043 mol = 21.3 J.
What are the units for standard Gibbs free energy?
The units for standard Gibbs free energy are joules per mole (J/mol) or kilojoules per mole (kJ/mol).
How much energy is generated from freezing 2.5 g water?
2.5 g 1 mol/18.02 g (-285.83) kJ/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
How do you Convert 40.79 kilojoules per mole to joules per grams?
To convert from kilojoules per mole to joules per gram, you need the molar mass of the substance. Once you have the molar mass, you can convert as follows: 1 kJ/mol = 1000 J/mol 40.79 kJ/mol = 40.79 * 1000 J/mol = 40790 J/mol Then, divide by the molar mass in grams/mol to get joules per gram.
How do I convert the enthalpy of vaporization of water in joules per gram from kiloJoules per mole?
Lets say, for example the enthalpy is equal to 1200 joules/gram. You take 1200 joules/gram * (# of grams)/one mole [now you can cancel grams and it is now joules/mole.] Then convert the answer to kilojoules by dividing by 1000.
What is the heat of solution for barium chloride in joules?
The heat of solution for barium chloride is -61.7 kJ/mol. To convert this to joules, multiply by 1000 to get -61,700 J/mol.
What is -1211.5 joules per kelvin converted to kilijoules per moles?
These are not compatible. The first is Energy per Temperature. The second is Energy per amount of matter.
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?
The first step is to calculate how many moles of Na are present in 1 mg (0.001 g) of Na. Since the molar mass of Na is 22.98977 g/mol, there are 0.000043 moles of Na. Next, convert the ionization energy to joules by multiplying by 1000 (1 kJ = 1000 J) to get 495,800 J/mol. Finally, multiply the number of moles by the energy per mole to find the total energy required: 495,800 J/mol * 0.000043 mol = 21.3 J.
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.
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.
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.
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 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 do you convert J per mol to J per Photon?
Multiply by avagardoes number
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.
