At `527^(@)C`, the reaction given below has`K_(c)=4`
`NH_(3)(g)hArr(1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)`
what is the `K_(p)` for the reaction ?
`N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g)`

For a reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g))

(K_(c))/(K_(p)) for the reaction, N_(2)(g)+3H_(2)(g)hArr2NH_(3(g)) is

At 527^@C , the reaction given below has K_c = 4 NH_3(g) iff 1/2 N_2(g) +3/2 H_2(g) What is the K_p for the reaction ? N_2(g) + 3H_2(g) iff 2NH_3(g)

For the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g), DeltaH=?

For the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g), DeltaH=?

Equilibrium constant K_(C) for the following reaction at 800 K is, 4 NH_(3)(g)hArr (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) . The value of K_(p) for the following reaction will be N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)

Equilibrium constant K_(C) for the following reaction at 800 K is, 4 NH_(3)(g)hArr (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) . The value of K_(p) for the following reaction will be N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)

Which of the following is correct for the reaction? N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g)