What mass of titanium chloride could be formed from the reaction of 3.00 g titan

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Explanation / Answer

Write a balanced equation Ti(s) + 2Cl2(g) ---------> TiCl4 2. Convert the mass of reagent to moles moles = mass / molar mass molar mass Cl2 = 70.9 g/mol molar mass Ti = 47.87 g/mol moles Ti = 3.00 g / 47.87 g/mol = 0.0627 mol moles Cl2 = 8.00 g / 70.9 g/mol = 0.113 mol 3. Work out the limiting reagent. This is the reagent that is not present in enough amounts to fully react all of the other reagent. The balanced equation shows that 1 moles Ti needs 2 mol Cl2 to fully react So 0.0627 mol Ti needs (2 x 0.0627) mol Cl2 = 0.1254 moles Cl2 needed to react all the Ti provided We have 0.113 mol of Cl2. This is less then 0.1254 moles, so there is not enough Cl2 for all the Ti. Thus Cl2 is the limiting reagent. 4. Determine moles of product formed. The maximum amount of product you can get is from complete reaction of all of the limiting reagent. This is because once the limiting reagent has been used up there can be no more product formed. The balanced equation shows that 2 moles Cl2 will react to give 1 moles TiCl4 So 1 mole Cl2 ----------> 1/2 mol TiCl4 Therefore 0.113 mole Cl2 ---------> (1/2 x 0.113)mol TiCl4 = 0.0565 moles TiCl4 will form 5. Convert back to mass moles = mass / molar mass therefore mass = molar mass x moles molar mass TiCl4 = 189.71 g/mol mass TiCl4 = 0.0565 mol x 189.71 g/mol = 10.7 g

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