2no2(g)⇌n2o4(g) kp=6.7at298k a 2.35-l container contains 0.053 mol of no2 and 0.084 mol of n2o4at298k. is the reaction at equilibrium? if not, in what direction will the reaction proceed?

Q> K hence the reaction proceeds in the reverse direction.

First we must obtain the concentration of each of the species;

NO2 - 0.053 mol/2.35-l = 0.023 M

N2O4 - 0.084 mol/2.35-l = 0.036 M

Hence;

Q = [N204]/[NO2]^2

Q = [0.036]/[0.023]^2

Q = 68.05

Since Q > K, it follows that the reaction moves towards the left hand side.

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1. 1 mole of anything contains 6.022x10^23 pieces  

d  

2. a  

3. c, number  

5. 1.24x10^24atoms / 6.022x10^23atoms/mole = 2moles h2 atoms  

6. fe2br3 mass = 2moles x mass fe + 3 moles x mass br  

molar mass = grams / number of moles = g/mole  

to find moles = g / molar mass  

to find mass = g = molar mass / moles

the dependant variable is spilled water

the independent is the heat