How much heat will be released when 1.48g of chlorine reacts with excess phosphorus according to the equation 2p+5cl2 2pcl5∆H=-886kj?

1 Answer
Write your answer here...
Start with a one sentence answer
Then teach the underlying concepts
Don't copy without citing sources
preview
?

Answer

Write a one sentence answer...

Answer:

Explanation

Explain in detail...

Explanation:

I want someone to double check my answer

Describe your changes (optional) 200

1
anor277 Share
Feb 9, 2018

Answer:

Slightly contrived circumstances here....

Explanation:

SO we gots #1/2P_4(s) +5Cl_2(g) rarr 2PCl_5# #DeltaH_"rxn as written"^@=-886*kJ*mol^-1#

The stated terms of the reaction are very poor. Phosphorus is likely to be oxidized to #PCl_3# or a lesser oxidation state in the presence of limited quantities of chlorine gas.

We assume that the reaction proceeds as written and a stoichiometric quantity of phosphorus reacts....

#"Moles of dichlorine"=(1.48*g)/(70.90*g*mol^-1)=0.0209*mol#...

And given the stoichiometry we gets...

#1/2xx0.0209*molxx(-886*kJ*mol^-1)=-9.25*kJ...#

Was this helpful? Let the contributor know!
1500