Chapter 6, Problem 6.89P

Consider the gas-phase reaction of ethylene $\left({\text{CH}}_{\text{2}}{\text{| |CH}}_{\text{2}}\right)$ with hydrogen to form ethane $\left({\text{C}}_{\text{2}}{\text{H}}_{\text{6}}\right)\text{,}$ which occurs in the presence of a palladium catalyst $\left(\text{Section-6}\text{.4B}\right)\text{.}$

1. Write the expression for the equilibrium constant for this reaction.
2. If $\Delta H=-\text{28 kcal,}$are the products or reactants higher in energy?
3. Which is likely to be true about the equilibrium constant for the reaction: $K>1$ or $K<1.$
4. How much energy is released when 20.0 g of ethylene reacts?
5. What happens to the rate of the reaction if the concentration of ethylene isincreased?
6. What happens to the equilibrium when each of the following changes occurs: $[1]$ an increase in ${\text{[H}}_{\text{2}}\text{]; [2]}$ a decrease in ${\text{[C}}_{\text{2}}{\text{H}}_6\text{]; [3]}$ an increase in temperature; $\text{[}4\text{]}$ an increase inpressure; $\text{[}5\text{]}$removal of the palladium catalyst?