Hydrocarbon reacts with oxygen to form carbon dioxide and water if it is complete combustion. But during incomplete combustion carbon mono oxide and water are formed.
The answer to this question is ZN2I
Answer:
14.0 g
Explanation:
Step 1: Write the balanced equation
2 Cu₂O + Cu₂S ⇒ 6 Cu + SO₂
Step 2: Calculate the moles corresponding to 10.5 g of copper (I) oxide
The molar mass of Cu₂O is 143.09 g/mol.
Step 3: Calculate the moles of copper produced from 0.0734 moles of copper (I) oxide
The molar ratio of Cu₂O to Cu is 2:6. The moles of Cu produced are 6/2 × 0.0734 mol = 0.220 mol
Step 4: Calculate the mass corresponding to 0.220 mol of copper
The molar mass of Cu is 63.55 g/mol.
Answer:
5.167 kJ
Explanation:
We have to divide the heating process into two steps: one for the heating process of liquid water (1) and the other for the phase transition from liquid water to steam at 100°C (2)
1 - heating from 52.1°C to 100°C:
heat(1) = m x Cp x ΔT = 2.1 g x 4.184 J/g°C x (100°C-52.1°C) = 420.9 J
2 - vaporization at 100°C:
heat(2) = m x ΔHv = 2.1 g x 2260 J/g = 4746 J
Finally, we add the heat values of the steps:
heat required = heat(1) + heat(2) = 420.9 J + 4746 J = 5166.9 J
Since 1 kJ= 1000 J, we convert from J to kJ:
5166.9 J x 1 kJ/1000 J = 5.1669 kJ ≅ 5.167 kJ