White phosphorous, P4(s) reacts with chlorine, Cl2(g) to form liquid phosphorus trichloride. a) Write a balanced...
White phosphorous, P4(s) reacts with chlorine, Cl2(g) to form liquid phosphorus trichloride.
a) Write a balanced equation.
b) What mass of phosphorous is required to react with excess chlorine to form 19.7g of phosphorous trichloride?
Homework Answers
A) balanced chemical reaction,
P4(s)+ 6Cl2(g) --->4PCl3(l)
B) molar mass of phosphorus trichloride =
137.5 g
Mass of P4 required=
= 4×31×19.7/4×137.5
=> 4.44 gc
Add Answer to:
White phosphorous, P4(s) reacts with chlorine, Cl2(g) to form
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