Question

Consider the reaction: B2H6(g) +3O2(g) ---> B2O3(s)+3H2O(g) ...........(triangle H) = -2035 KJ Calculate the amount of...

Consider the reaction:

B2H6(g) +3O2(g) ---> B2O3(s)+3H2O(g) ...........(triangle H) = -2035 KJ

Calculate the amount of heat released when each of the following amounts of diborane (B2H6) is burned

-1.000 x 10^2 mol

-1 mol

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Answer #1

B2H6(g) + 3O2(g) -----> B2O3(s) + 3H2O(g)          H = -2035 KJ

from the balanced equation 1 mole of B2H6 gives ----> 2035KJ energy.

then 1.000*10^2 moles of B2H6 gives -----> 100*2035 KJ

                                                                = 203500 KJ

H = - 203500 KJ

then 1 mole of B2H6 gives -------> 2035 KJ

H = -2035 KJ

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