The reaction between potassium chlorate and red phosphorus takes place when you

Question

The reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 64.5 g of potassium chlorate (KClO3) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P4O10) could be produced?
KClO3 (s) + P4(s) --> P4O10 (s) + KCl(s) (Unbalanced)
Mass (g) = ? t.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do locator-assignment-take&takeAssignmentSession; ocator assignment-take The reaction between potassium chlorate and red phosphorus takes place when you strike potassium a match on a matchbox. If you were to react 64.5 g of chlorate (KCIOs) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P4O1o) could be KCIOs(s) + P1(s) P,010 (s) + KCl(s) (unbalanced) produced? Mass Submit Answer Try Another Version 9 item attempts remaining

Explanation / Answer

Balanced reaction:

10 KClO3(s) + 3 P4(s) = 3 P4O10(s) + 10 KCl(s)
Molar mass of KClO3: 122.6 g/mol
Moler mass of P4: 123.9 g/mol
Moler mass of P4O10: 283.9 g/mol
From balanced reaction, 10 x 122.6 = 1266 g of KClO3 is required to produce 3 x 283.9 = 851.7 g of P4O10
Hence, P4O10 produced from 64.5 g of KClO3 = 64.5 x 851.7 / 1266
= 43.39
= 43.4 g of P4O10

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