Is the haber process for the industrial synthesis of ammonia spontaneous or nonspontaneous under standard conditions at 25 ∘c? n2(g)+3h2(g)→2nh3(g) δh∘=−92.2 kj; δs∘=−199 j/k?

The  industrial  synthesis  of  ammonia   is  spontaneous.

 to  to  prove this  one  calculate  the  gibbs  free  energy(delta G)

=   delta  G  =  Delta  H  -T delta  s

delta H = -92.2  kj  in  joules  -92.2  x1000 =-92200j
delta  s  =  -199j/k
T=  25+273=  298k

delta  G  is  therefore=   -92200-298(-199)=-32898j
since  delta G  is  negative the  reaction  is  therefore  spontaneous

m=9

step-by-step explanation:

7m+8=71 subtract   8 from 71 which is 63 than divide it by 7m   equal 9.