Answer:
Tin(IV) Hydrogen Oxalate. Alias: Stannic Hydrogen Oxalate. Formula: Sn(HC2O4)4. Molar Mass: 474.8178. :: Chemistry Applications:: Chemical Elements, Periodic Table.
Explanation:
The molar enthalpy of combustion in kj/mol of magnesium is 620 kj/mol, Option D is the correct answer.
<h3>What is enthalpy of Combustion ?</h3>
The energy released when a fuel is oxidized by an oxidizing agent is called enthalpy of Combustion.
It is given that
a 1.0 g sample of magnesium is burned to form MgO. in doing so, 25.5 kj of energy are released.
Molecular weight of Magnesium = 24.35g
24.35 g makes 1 mole of Mg
1g = 1/24.35
For 0.04 moles 25.5 kJ is released
for 1 mole 25.5 *1/.04
= 620 kj/mol
Therefore the molar enthalpy of combustion in kj/mol of magnesium is 620 kj/mol.
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For every 1 mole of C6H12O6, you need 6 moles of water. Multiply the 2.5 moles you are trying to make by the 6 of water you need, and 4) 15 is your answer.
