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The balanced reaction is as below
3A₂B + 2DC₃→ 6 AC + D₂B₃
The number that must be to the left of AC is 6
Explanation
- According to the law of mass conservation , the number of atoms in reactant side must be equal to number to the number of atoms in product side.
- Therefore the equation above is balance since it obey the law of mass conservation.
- For example there is 6 atoms of A in reactant side and 6 in product side.
Answer:
Trial Number of moles
1 0.001249mol
2 0.001232mol
3 0.001187 mol
Explanation:
To calculate the <em>number of moles of tritant</em> you need its<em> molarity</em>.
Since the<em> molarity</em> is not reported, I will use 0.1000M (four significant figures), which is used in other similar problems.
<em>Molarity</em> is the concentration of the solution in number of moles of solute per liter of solution.
In this case the solute is <em>NaOH</em>.
The formula is:
![Molarity=\dfrac{\text{Number of moles of solute}}{\text{Volume of solution in liters}}](https://tex.z-dn.net/?f=Molarity%3D%5Cdfrac%7B%5Ctext%7BNumber%20of%20moles%20of%20solute%7D%7D%7B%5Ctext%7BVolume%20of%20solution%20in%20liters%7D%7D)
Solve for the <em>number of moles:</em>
![\text{Number of moles}=Molarity\times Volume\text{ }in\text{ }liters](https://tex.z-dn.net/?f=%5Ctext%7BNumber%20of%20moles%7D%3DMolarity%5Ctimes%20Volume%5Ctext%7B%20%7Din%5Ctext%7B%20%7Dliters)
Then, using the molarity of 0.1000M and the volumes for each trial you can calculate the number of moles of tritant.
Trial mL liters Number of moles
1 12.49 0.01249 0.01249liters × 0.1000M = 0.001249mol
2 12.32 0.01232 0.01232liters × 0.1000M = 0.001232mol
3 11.87 0.01187 0.01187liters × 0.1000M = 0.001187 mol
5 hope this helps I’m pretty sure it should be right