If you have 730 moles of a gas at 304 Kelvin in a 4.50 Liter container what
1 answer:
Answer:
4046atm
Explanation:
For this question you can use the ideal gas law,
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Where P is pressure, V is volume, n is moles of substance, R is the constant, and T is the temperature.
Because of the units given, R will equal .08026
Then, plug in the values (I'll be excluding units for simplicity, but they all cancel out for pressure in atm):
This will give you:
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The energy absorbed by the system before the reaction start has been 752 kJ/mol.
The bond energy has been defined as the energy possessed by the bond that has been converted into the heat energy and utilized in the reaction.
The energy has been conserved in a chemical reaction. Thus, the energy absorbed by the reactant in the reaction has been the difference in the energy of the reactant and product.
<h3>Computation for the energy absorbed</h3><h3 />The given reaction has been:
The bond energy of the reactant has been:
H-H bond energy = 432 kJ/mol
2 C=O bond energy= 799 kJ/mol
The total energy of the reactant has been 432 kJ/mol + 799 kJ/mol
The total energy of the reactant has been 1231 kJ/mol
The bond energy of the product has been:
C-O bonds = 358 kJ/mol
C=O bonds = 745 kJ/mol
1 C-H bond = 413 kJ/mol
1 O-H bond = 467 kJ/mol
The total energy of the product has been 358 + 745 + 413 + 467 kJ/mol
The total energy of the product has been 1,983 kJ/mol
According to the law of conservation of energy:
Substituting the values for energy absorbed:
The energy absorbed by the system before the reaction start has been 752 kJ/mol.
Learn more about bond energy, here: