Asample of nitrogen gas at 25°c and 745 mm hg has a volume of 35.0 l. what volume will it occupy if the pressure rises to 1125 mm hg at constant temperature? 1 atm = 760 mm hg.

The  volume that is occupied  if the  pressure   rises to 1125 mmHg  at  constant temperature  is  23.18 L

       calculation
This is calculated  using the Boyles   law formula  since the temperature  is constant
That is  P1v1 =P2V2
P1=745  mm hg
v1= 35.0 L
P2=1125  mm hg
V2=?

by making  V2  the subject of the formula  V2 = P1V1/P2

V2  is therefore =  (745  mmhg  x  35 L) / 1125 mm hg  = 23.18 L

Only one reactant yields 2 or more products. meaning you will only have 1 product and it will break down into 2 or more products. eg. h2o -> h2 + o2

Qand k are only the same when the forward rate of the reaction has reached zero.