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Calculate the heat evolved when 266 g of white phosphorus
Chapter 6, Problem 3PE(choose chapter or problem)
QUESTION:
Calculate the heat evolved when 266 g of white phosphorus \(\left(P_{4}\right)\) burns in air according to the equation
\(P_{4}(s)+5 O_{2}(g) \rightarrow P_{4} O_{10}(s)\) \(\Delta H=-3013 \mathrm{~kJ} / \mathrm{mol}\)
Questions & Answers
QUESTION:
Calculate the heat evolved when 266 g of white phosphorus \(\left(P_{4}\right)\) burns in air according to the equation
\(P_{4}(s)+5 O_{2}(g) \rightarrow P_{4} O_{10}(s)\) \(\Delta H=-3013 \mathrm{~kJ} / \mathrm{mol}\)
ANSWER:
Step 1 of 2
The given reaction is as follows.
From the above reaction phosphorous burns in air it forms tetraphosphorus decoxide.
And from the thermochemical equation 3013 kJ of heat is evolved per mole of reacted.