The reaction between titanium ( IV) oxide and bromine trifluoride to give liquid bromine , and oxygen is:

Thus from each three moles of titanium ( IV) oxide we will get three moles of oxygen molecule
The mass of oxygen obtained = 0.143g
The moles of oxygen obtained
= 
So moles of titanium ( IV) oxide required will be 0.00447mol
the molar mass of titanium ( IV) oxide is 79.87g/mol
mass of titanium ( IV) oxide used will be = 
This mass of titanium ( IV) oxide is present in 2.367g of impure sample
the mass percent will be


The percentage of titanium ( IV) oxide in impure sample is 15.08% (w/w)
Answer:
When the solution turns clear, either at the end of the reaction or when you add sufficient cyclohexene
Explanation:
The colour of bromine in the solution is usually yellow, however when the solution turns clear, this shows that all the bromine has been consumed.
Another way to make sure that all the bromine molecules are consumed is by addition of an unsaturated hydrocarbon like cyclohexene. Cyclohexene will consume the bromine molecules and the solution will become clear, while the cyclohexene becomes more saturated by becoming bromo cyclohexane.
Answer:
1. 1.100x10⁴mg
2. 2444mg
Explanation:
1. The 18.00g milk chocolate bar contain 11.00g of sugar. In miligrams:
11.00g * (1000mg / 1g) = 1.100x10⁴mg
2. If a bar of 18.00g contain 11.00g of sugar, a bar of 4.000g will contain:}
4.000g bar * (11.00g / 18.00g) = 2.444g of sugar.
In miligrams:
2.444g * (1000mg / 1g) = 2444mg