Question #67d90

1 Answer
Apr 10, 2017

Answer:

7540 torr

Explanation:

#K_p =(P_(NOBr) )^2/[(P_(Br_2))(P_(NO))^2 #
The exponents were determined from the coefficients in front of each product or reactant. Also the equilibrium constant is #(Products)/(Reactants)# as can be seen with how the equilibrium constant is written. Now we just plug in and solve for the partial pressure of NOBr

#28.4 =(P_(NOBr) )^2/[(154)(114)^2] #

#P_(NOBr)#=7539.185 torr

Rounded according to significant figures: 7540 torr