Question #353c0

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Answer 1 · 2017-03-17T05:27:34

#K_p = 2.25#

#Delta_r G= Delta_r G^0 + RT ln Q#

The reaction is occurring at standard conditions then #Delta_r G^0=0# and #Q= K_(eq)#

#Delta_r G= RT ln Q#

#176.31 = 0.0821 xx 298 xx ln Q#

# ln Q = 7.2063#

# Q =1347.895#

# Q =K_(eq)=1347.895#

#K_p = K_c (RT)^(Delta ng)#

#K_p = 1347.895xx (0.0821 xx 298)^(-2)#

#K_p = 1347.895xx (24.4658)^(-2)#

#K_p = 1347.895/ (24.4658)^(2)#

#K_p = 1347.895/ 598.5753#

#K_p = 2.2518#

#K_p = 2.25#