To find the bond energy of H-H, we need to calculate the energy consumed in breaking the H-H bond.
The energy required to dissociate 8.000 g of gaseous Hydrogen into free gaseous atoms is 873.6 kJ. The molar mass of hydrogen is 2.016 g/mol.
First, we need to calculate the moles of hydrogen.
Number of moles = mass / molar mass = 8.000 g / 2.016 g/mol = 3.97 mol
The bond energy is the energy required to break one mole of H-H bonds, so we divide the total energy by the number of moles.
Bond energy = Total energy / Moles of hydrogen = 873.6 kJ / 3.97 mol ≈ 219.6 kJ/mol
Therefore, the bond energy of H-H is approximately 219.6 kJ/mol.
Among the given options, the closest value to this is 220.5 kJ (option d).
The energy required to dissociate 8.000 g of gaseous Hydrogen into free gaseous atom is 873.6 kJ at 25.00 °C.
The bond energy of H-H will be
Question 2 options:
a) 200.0 kJ
b) 215.5 kJ
c) 175.3 kJ
d) 220.5 kJ
e) 218.4 kJ
5 answers
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Apologies for the confusion. Let's recalculate.
The energy required to dissociate 8.000 g of gaseous hydrogen into free gaseous atoms is 873.6 kJ. The molar mass of hydrogen is 2.016 g/mol.
First, we need to calculate the moles of hydrogen.
Number of moles = mass / molar mass = 8.000 g / 2.016 g/mol = 3.97 mol
The bond energy is the energy required to break one mole of H-H bonds, so we divide the total energy by the number of moles.
Bond energy = Total energy / Moles of hydrogen = 873.6 kJ / 3.97 mol ≈ 220.0 kJ/mol
Therefore, the bond energy of H-H is approximately 220.0 kJ/mol.
Based on the available answer choices, the closest value is 220.5 kJ (option d).
The energy required to dissociate 8.000 g of gaseous hydrogen into free gaseous atoms is 873.6 kJ. The molar mass of hydrogen is 2.016 g/mol.
First, we need to calculate the moles of hydrogen.
Number of moles = mass / molar mass = 8.000 g / 2.016 g/mol = 3.97 mol
The bond energy is the energy required to break one mole of H-H bonds, so we divide the total energy by the number of moles.
Bond energy = Total energy / Moles of hydrogen = 873.6 kJ / 3.97 mol ≈ 220.0 kJ/mol
Therefore, the bond energy of H-H is approximately 220.0 kJ/mol.
Based on the available answer choices, the closest value is 220.5 kJ (option d).
are you still sure, bot?
Apologies for the mistake in my previous response. Let's recalculate the bond energy correctly.
Given:
Energy required to dissociate 8.000 g of gaseous Hydrogen = 873.6 kJ
First, we need to calculate the moles of hydrogen. The molar mass of hydrogen is 2.016 g/mol.
Number of moles = mass / molar mass = 8.000 g / 2.016 g/mol = 3.97 mol
To find the bond energy, we need to divide the energy consumed by the number of moles of hydrogen.
Bond energy = Energy consumed / Number of moles = 873.6 kJ / 3.97 mol ≈ 219.8 kJ/mol
Based on the available answer choices, the closest value to the bond energy is 220.5 kJ (option d).
Given:
Energy required to dissociate 8.000 g of gaseous Hydrogen = 873.6 kJ
First, we need to calculate the moles of hydrogen. The molar mass of hydrogen is 2.016 g/mol.
Number of moles = mass / molar mass = 8.000 g / 2.016 g/mol = 3.97 mol
To find the bond energy, we need to divide the energy consumed by the number of moles of hydrogen.
Bond energy = Energy consumed / Number of moles = 873.6 kJ / 3.97 mol ≈ 219.8 kJ/mol
Based on the available answer choices, the closest value to the bond energy is 220.5 kJ (option d).
2 answers