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You are given a 10.00 gram solid mixture of [tex]Ca(ClO_3)_2[/tex] and [tex]Ca(ClO)_2[/tex]. When this mixture is heated, both componds decomplse, releasing oxygen gas and leaving behind solid [tex]CaCl_2[/tex]

When this 10.00gram mixture is sealed in a 10.0-Liter evacuated vessel and heated to 700C, both compounds completely decompose according to the above reactions. The final pressure in the vessel is 1.00atm. Determine the mass of each compound in the original mixture.

Ok. I have written out the balanced equation of the two substances:

[tex] Ca(ClO_3)_2 + O_2 --> CaCl_2 + 4O_2[/tex] and

[tex] Ca(ClO)_2 + O_2 --> CaCl_2 + 2O_2[/tex]

using the ideal gas law, i have found that the total [tex]O_2[/tex] collected is 0.1252 mol (V = 10L , T = 973K, P = 1.00atm)

so I have let x equal to the gram of [tex]Ca(ClO_3)_2[/tex] and y equal to the gram of [tex]Ca(ClO)_2[/tex], combine them toegether, I have:

x + y = 10

and then i found out the precentage of O2 that each substance produce, so I have another equation:

(0.0193) x + (0.0186) y = 0.1252

when i solve for x and y , i have x equal to -86 and y = 96, which obviously, is not possible?

Any clues on how to solve this probelm?