Answer:
3189.07Pa
Explanation:
The conversion of 23.92mmH to Pa can be achieved in the following way:
760mmHg = 101325Pa
23.92mmHg = (23.92x101325)/760 = 3189.07Pa
Answer:
21.4 L
Explanation:
Given data:
Volume of carbon dioxide produced = ?
Volume of oxygen = 37.4 L
Solution:
Chemical equation:
2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O
It is known that,
1 mole = 22.414 L
There are 7 moles of oxygen = 7×22.414 = 156.9 L
There are 4 moles of carbon dioxide = 4×22.414 = 89.66 L
Now we will compare:
O₂ : CO₂
156.9 : 89.66
37.4 : 89.66/156.9×37.4 = 21.4 L
So from 37.4 L of oxygen 21.4 L of carbon dioxide is produced.
Atoms tend to form bonds because one atom may have more attraction to electrons than the other<span />
Answer:
The limiting reactant is AlCl₃ and the excess reactant is NaOH.
Explanation:
- The balanced equation for the mentioned reaction is:
<em>3NaOH(aq) + AlCl₃(aq) → 3NaCl(aq) + Al(OH)₃(s)↓,</em>
It is clear that 3.0 moles of NaOH(aq) react with 1.0 mole of AlCl₃(aq) to produce 3.0 moles of NaCl(aq) and 1.0 mole of Al(OH)₃(s).
- Firstly, we need to calculate the no. of moles of (8.0 g) of NaOH and (4.0 g) of AlCl₃:
no. of moles of NaOH = mass/molar mass = (8.0 g)/(40.0 g/mol) = 0.2 mol.
no. of moles of AlCl₃ = mass/molar mass = (4.0 g)/(133.34 g/mol) = 0.03 mol.
- From stichiometry; NaOH reacts with AlCl₃ with (3: 1) molar ratio.
∴ 0.09 mol of NaOH (the remaining 1.1 mol is in excess) reacts completely with 0.03 mol of AlCl₃.
<em>the limiting reactant is AlCl₃ and the excess reactant is NaOH.</em>
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Answer:
375.3KJ
Explanation:
The following data were obtained from the question:
Mass of water = 166g
Heat of Vaporisation (ΔHv) = 40.7kJ/mol
Heat (Q) =..?
Next, we shall determine the number of mole in 166g of water. This is illustrated below:
Mass of H2O = 166g
Molar mass of H2O = (2x1) + 16 = 18g/mol
Number of mole = Mass/Molar Mass
Number of mole of H2O = 166/18
Number of mole of H2O = 9.22 moles.
Now, we can obtain the heat required to vaporise the water as shown below:
Q = n·ΔHv
Q = 9.22 mol x 40.7kJ/mol
Q = 375.3KJ
Therefore, the heat required to vaporise the water is 375.3KJ.
