4Fe(s) + 3O2(g) → 2Fe2O3(s) ....... ΔH = -1.7 x 10^3 kJ
<span>shows that 1700 kJ of heat is released when 4 moles of Fe react. </span>
<span>Molar mass of Fe = 56 g/mol </span>
<span>Molar mass of Fe2O3 = 160 g/mol. </span>
<span>(a) When 4 mol ( 4 x 56 = 224 g) iron reacted 1700 kJ are released, </span>
<span>when 9.0 g Fe reacted, the amount of energy will be </span>
<span>(9.0 x 1700) / (224) = 68.3 kJ </span>
<span>(b) According to the equation, 1700 kJ of energy released during the formation of 2 moles of Fe2O3 which is 2 x 160 = 320 g of rust. </span>
<span>120 kcal x (4.18 kJ / 1 kcal) = 501.6 kJ </span>
<span>When 1700 kJ released = 320 g rust </span>
<span>when 501.6 kJ released = (501.6 x 320) / 1700 = 94.4 g rust</span>
Answer:
Where is your question? I do not see it.
Explanation:
Answer:
3520 g of CO₂
Explanation:
2C₂H₆ + 70₂ → 4CO₂ + 6H₂O
molar ratio of the above reaction is;
2 : 7 → 4 : 6
2 moles of C₂H₆ will form 6 moles of H₂O
Thus, 1 mole of C₂H₆ will form 3 moles of H₂O
mass of H₂O = 360 g
molecular weight of H₂O = 18 g/mol
molar mass = mass ÷ molecular weight = 360÷18 = 20 moles
Total number of moles of H₂O formed = 6 * 20 moles = 120 moles
Number of moles of C₂H₆ reacted = 120 moles ÷ 3 = 40 moles
molar ratio of C₂H₆ to CO₂ = 1 : 2
Thus, number of moles of CO₂ formed = 2 * 40 moles = 80 moles
molecular weight of CO₂ = 44 g/mol
mass of CO₂ formed = number of moles x molecular weight = 80 * 44 = 3520 g
Answer:
See explanation
Explanation:
The law of conservation of mass states that mass can neither be created nor destroyed. This implies that in a chemical reaction, we can only have the same number of atoms of each element on both sides of the reaction equation.
If we write 4Fe2S3 it means that we have;
4 * 2 = 8 atoms of Fe
4 * 3 = 12 atoms of S
8 + 12 = 20 atoms in all