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olganol [36]
3 years ago
7

What is the mole ratio to correct balance the reaction below? __KBr + __Ca3N2--> __CaBr2 + __K3N

Chemistry
1 answer:
jonny [76]3 years ago
7 0

Explanation:

3CaBr2 + 2K3N → 6KBr + Ca3N2

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For the reaction Fe3O4(s) + 4H2(g) --> 3Fe(s) + 4H2O(g)
mojhsa [17]

Answer : The value of equilibrium constant for this reaction at 328.0 K is 1.70\times 10^{15}

Explanation :

As we know that,

\Delta G^o=\Delta H^o-T\Delta S^o

where,

\Delta G^o = standard Gibbs free energy  = ?

\Delta H^o = standard enthalpy = 151.2 kJ = 151200 J

\Delta S^o = standard entropy = 169.4 J/K

T = temperature of reaction = 328.0 K

Now put all the given values in the above formula, we get:

\Delta G^o=(151200J)-(328.0K\times 169.4J/K)

\Delta G^o=95636.8J=95.6kJ

The relation between the equilibrium constant and standard Gibbs free energy is:

\Delta G^o=-RT\times \ln k

where,

\Delta G^o = standard Gibbs free energy  = 95636.8 J

R = gas constant  = 8.314 J/K.mol

T = temperature  = 328.0 K

K = equilibrium constant = ?

Now put all the given values in the above formula, we get:

95636.8J=-(8.314J/K.mol)\times (328.0K)\times \ln k

k=1.70\times 10^{15}

Therefore, the value of equilibrium constant for this reaction at 328.0 K is 1.70\times 10^{15}

3 0
3 years ago
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