Answer:
144g of H₂O
Explanation:
3NH₄ClO₄(s) + 3Al → Al₂O₃(s) + AlCl₃(s) + 3NO(g) + 6H₂O(g)
From the equation:
3 moles of NH₄ClO₄ produced 6 moles of H₂O
4 moles of NH₄ClO₄ produced ? moles of H₂O
(4 ₓ 6)/3 = 
= 8 moles of H₂O
1 mole of H₂O = (1 × 2) + 16 = 18g (The Relative Molecular mass of H₂O)
8 moles of H₂O = ?
Therefore 8 × 18 = 144g
=144g of H₂O
In this item, I supposed, that we are determine the molar fraction of oxygen and carbon dioxide in the sample. This can be done by dividing their respective partial pressures by the total pressure of the sample.
O2 : mole fraction = (100.7 mmHg) / (763.00 mmHg) = 0.13
CO2 : mole fraction = (33.57 mmHg) / (763.00 mmHg) = 0.044
Answers: O2 = 0.13
CO2 = 0.044
Answer:
Explanation:
Standard enthalpy of combustion (ΔH∘C) is the enthalpy change when 1 mole of a substance burns under standard state conditions;
Its TRUE because the hypothesis is only true when you have facts behind it has to be testable
The balanced chemical reaction is
NaCl + AgNO3 --> AgCl + NaNO3
To find out if precipitation will occur, we need to calculate the number of
moles acting in the chemical reaction
But Molarity, M=nV, where n is the number of moles and V is the volume in
litres. So n = M/V
number of moles of AgNo3 = 0.02/500 * 10^(-3)
n= 0.04
While n of Sodium chloride = 0.01/0.5 = 0.2. Since there is excess sodium chloride ( twice as much) precipitation will not occur. 2NaCl + 2AgNO3 -->
2AgCl + 2NaNO3. The reaction requires one and not two moles of AgNo3 as evident from the number of moles which is 0.04
