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How many kilojoules or energy are required to vaporize 5 g of ethane?
The heat of vaporization for ethane is approximately 16.7 kJ/g. Therefore, to vaporize 5 g of ethane, the energy required would be: 16.7 kJ/g * 5 g = 83.5 kJ.
How much energy is generate from freezing 2.5 g water?
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
What is the value for G at 700 K if H -92 kj mol and S -0.199 kj mol-k?
To calculate the Gibbs free energy (G) at 700 K, we can use the formula: ( G = H - TS ). Given that ( H = -92 , \text{kJ/mol} ) and ( S = -0.199 , \text{kJ/(mol·K)} ), we first calculate ( TS = 700 , \text{K} \times -0.199 , \text{kJ/(mol·K)} = -139.3 , \text{kJ/mol} ). Then, substituting into the Gibbs equation: [ G = -92 , \text{kJ/mol} - (-139.3 , \text{kJ/mol}) = 47.3 , \text{kJ/mol}. ] Thus, the value for G at 700 K is 47.3 kJ/mol.
How much heat is produced when 4.6 g of butane is completely combusted in air?
The heat produced when 1 mole of butane is completely combusted is -2877 kJ. The molar mass of butane is 58.12 g/mol, so 4.6 g is 0.079 moles. Therefore, the heat produced when 4.6 g of butane is combusted is -227.1 kJ.
How much heat is required to melt 98.5 g of ice at its melting point?
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)
How many kilojoules or energy are required to vaporize 5 g of ethane?
The heat of vaporization for ethane is approximately 16.7 kJ/g. Therefore, to vaporize 5 g of ethane, the energy required would be: 16.7 kJ/g * 5 g = 83.5 kJ.
How much energy in kJ is needed to melt 183.3 g of water at 0 C?
The energy needed to melt ice is given by the formula Q = m * L_f, where Q is the energy required, m is the mass of water, and L_f is the heat of fusion of water (334 J/g). Converting 334 J/g to kJ/g gives 0.334 kJ/g. Multiplying these together, we find that 183.3 g of water will require 61.21 kJ of energy to melt at 0°C.
What is the value for G at 100 K if H 27 kJmol and S 0.09 kJ(molK)?
The equation relating G, H, and S is G = H - TS, where T is the temperature in Kelvin. Plugging in the values given, G = 27 kJ/mol - 100 K * 0.09 kJ/(molK) = 27 kJ/mol - 9 kJ/mol = 18 kJ/mol. So, the value for G at 100 K is 18 kJ/mol.
What is the value for G at 100 K if H 27 kJ mol and S 0.09 kJ molK?
G=18 kJ/mol
How much ice is consumed by thawing 4.3 g ice?
4.3 g * 1 mol/18.02 g * 6.03 kJ/mol
How much energy is generate from freezing 2.5 g water?
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
How much g's doe's the bakugan Griffon have?
It can have up to 450 g's depending on the Attribute.
1: At which temperature would a reaction withΔH = -102 kJ/mol, ΔS = -0.188 kJ/(mol×K) be spontaneous2:At which temperature would a reaction withΔH = 132 kJ/mol, ΔS = 0.200 kJ/(mol×K) be spontaneous?
Using the following thermochemical data, what is the change in enthalpy for the following reaction: 3H2(g) + 2C(s) + ½O2(g) → C2H5OH(l) C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l), ΔH = –1367 kJ/mol C(s)+O2(g)→CO2(g), ΔH = –393.5 kJ H2(g)+½O2(g)→H2O(l), ΔH = –285.8 kJ a. -277.6 kJ/mol b. -194.7 kJ/mol c. 194.7 kJ/mol d. 486 kJ/mol
How much energy is absorbed when 356 g of ethanol 46.0 gmol boils?
The heat of vaporization of ethanol is 38.6 kJ/mol-298 - 299 KJ
What is the value for G at 100 K if H equals 27 kJ mol and S equals 0.09 kJ molK?
To find the value of G at 100 K, you can use the equation ΔG = ΔH - TΔS. Plugging in the values, you get ΔG = 27 kJ/mol - (100 K)(0.09 kJ/molK) = 18 kJ/mol. Therefore, the value for G at 100 K would be 18 kJ/mol.
What is the value for G at 300 K if H 27 kJmol and S 0.09 kJmolK?
G = 0 kJ/mol
What is the value for g at 5000 k if h -220 kj mol and s equals -0.05 kj molk?
-18 kj/mol
