Heating 2.40 g of the oxide of metal X (molar mass of X=55.9g/mol) in carbon mon
ID: 685469 • Letter: H
Question
Heating 2.40 g of the oxide of metal X (molar mass of X=55.9g/mol) in carbon monoxide yields the pure metal and carbondioxide. the mass of the mtal product is 1.68g. From the datagiven, show that the simplest formula of the oxide isX2O3. I was only able to find the moles of X and I got stuck afterthat. I'm not sure how to find XyOz toprove the simples formula is X2O3 Heating 2.40 g of the oxide of metal X (molar mass of X=55.9g/mol) in carbon monoxide yields the pure metal and carbondioxide. the mass of the mtal product is 1.68g. From the datagiven, show that the simplest formula of the oxide isX2O3. I was only able to find the moles of X and I got stuck afterthat. I'm not sure how to find XyOz toprove the simples formula is X2O3Explanation / Answer
From the given information, The number of moles of product 'X' formed = 1.68 g /55.9 g/mol = 0.03 moles Since the number of moles of the X in product = numberof moles X of the reactant The same number of moles of X in the reactant also 0.03moles Therefore mass of O in the reactant = 2.40 g -1.68 g =0.72 g Threrefore number of moles of the reactant = 0.72 g/16.0g/mol = 0.045 mol Therefore empirical formula of the compound iscalculated as follows. X O 0.03 0.045 0.03/0.045 0.045/0.045 0.66 1 By multyiplying with factor 3 we get the - 2 3 Therefore simplestformula of the compound = X2O3.Related Questions
Hire Me For All Your Tutoring Needs
Integrity-first tutoring: clear explanations, guidance, and feedback.
Drop an Email at
drjack9650@gmail.com
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.