2. Consider the following equilibrium 2502 (g) + O2 (g) 2SO3 (g) From which of t

Question

2. Consider the following equilibrium 2502 (g) + O2 (g) 2SO3 (g) From which of the following starting conditions would it be impossible for this equilibrium to be achieved? a) 0.25 mol SO2 (g) and 0.25 mol O2 (g) are in a 1.0L container. b) 0.75 mol SO2 (g) in al.OL container. c) 0.50 mol O2 (g) and 0.50 mol SO3 (g) in al.OL container. d) 1.0 mol SOs (g) in 1.OL container 3. Which statement is incorrect? a) b) c) Le Chatelier's Principle predicts which action(s) below to cause the endothermic half-life of a first order reaction is directly proportional to the initial concentration half-life of a second order reaction is inversely proportional to the initial concentration half-life of a first order reaction is independent of the initial concentration 4. reaction CH3CH-CH2 (g) C3H6 (g) to form more CH3CH-CH2 than initially present at equilibrium? a) increasing the system temperature b) decreasing the system temperature c) increasing the system pressure d) decreasing the system pressure e) decreasing both the system pressure and the system temperature

Explanation / Answer

2) As the mol of SO2 and SO3 cant be same thats why it is   impossible for equilibrium.

3)half life of the 1st order reaction does not depend on the initial concentration.

4)change in H=+ve

then , CH3CH=CH2+heat =>C3H6

If we increase temperature then it will go backward.

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