i was told to Convert 1 metric ton to grams ore then to grams TiO2 (using the 0.75% in the ore), then to g TiCl4 (using the 70%%) and finally to TiO2 final product (using the 93.0%)for the following questions, but im stuck after converting the metric ton to grams
About half the world's production of pigments for paints involves the formation of white TiO2. It is made on a large scale by the chloride process , starting with ores containing only small amounts of rutile, TiO2. The ore is treated with chlorine and carbon. this produces TiCl4 and gaeseous product according to the following equation:
3TiO2(s)+ 4C(s)+ 6Cl2(g)--> 3TiCl4(l)+ 2CO2(g)+ 2CO(g)
the titanium(IV)chloride is then converted into titanium(IV)oxide of high purity
TiCl4(l)+ O2(g)--> TiO2(s)+ 2Cl2(g)
suppose the first process can be carried out with 70.0% yield and then second one with 93.0% yield. How many kilograms of TiO2 could be produced starting with 1.00metric ton (1.00x10^6g)of an ore that is 0.75% rutile TiO2?
After you have grams TiO2 in the ore, use the stoichiometry procedure I posted for you. That procedure will convert TiO2 to TiCl4.
Here is the procedure again.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To solve this problem, we need to convert the 1 metric ton (1.00 x 10^6 g) of ore to grams of titanium dioxide (TiO2), using the given information. Let's break down the problem step by step:
Step 1: Convert 1 metric ton to grams:
1 metric ton = 1000 kg
1 kg = 1000 g
Therefore, 1 metric ton = 1000 kg x 1000 g = 1.00 x 10^6 g
Now that we have the mass of the ore in grams, we can proceed to the next step.
Step 2: Calculate the grams of rutile TiO2 in the ore:
The ore contains 0.75% rutile TiO2. To determine the grams of rutile TiO2, we multiply the mass of the ore by the percentage of rutile TiO2:
Grams of rutile TiO2 = Mass of ore x Percentage of rutile TiO2
= 1.00 x 10^6 g x 0.75%
= 1.00 x 10^6 g x 0.0075
= 7.50 x 10^3 g
Now, we have the grams of rutile TiO2 in the ore.
Step 3: Calculate the grams of TiCl4 produced from the rutile TiO2:
The stoichiometry of the reaction shows that 3 moles of TiO2 produce 3 moles of TiCl4. Since the molar mass of TiO2 is 79.87 g/mol and the molar mass of TiCl4 is 189.7 g/mol, we can use these values to convert grams of rutile TiO2 to grams of TiCl4.
Grams of TiCl4 = Grams of rutile TiO2 x (1 mol TiCl4 / 3 mol TiO2) x (189.7 g TiCl4 / 1 mol TiCl4)
= 7.5 x 10^3 g x (1 / 3) x (189.7 g / 1)
= 4.7485 x 10^5 g
= 4.7485 x 10^5 g (rounded to four decimal places)
Now, we have the grams of TiCl4 produced from the rutile TiO2 in the ore.
Step 4: Calculate the grams of TiO2 produced from TiCl4:
The second reaction states that 1 mol of TiCl4 produces 1 mol of TiO2. Again, using the molar masses of TiCl4 (189.7 g/mol) and TiO2 (79.87 g/mol), we can convert the grams of TiCl4 to grams of TiO2.
Grams of TiO2 = Grams of TiCl4 x (1 mol TiO2 / 1 mol TiCl4) x (79.87 g TiO2 / 1 mol TiO2)
= 4.7485 x 10^5 g x (1 / 1) x (79.87 g / 1)
= 3.795 x 10^7 g
= 3.795 x 10^7 g (rounded to three decimal places)
Finally, we have the grams of TiO2 produced from TiCl4.
Step 5: Convert grams to kilograms:
To convert the grams of TiO2 to kilograms, we divide by 1000.
Kilograms of TiO2 = Grams of TiO2 / 1000
= 3.795 x 10^7 g / 1000
= 3.795 x 10^4 kg
= 37,950 kg
Therefore, starting with 1.00 metric ton of ore that is 0.75% rutile TiO2, you could produce approximately 37,950 kilograms of TiO2.