Hydrogen for this reaction may be prepared by reacting methane with steam, and carbon monoxide is also produced in the process. Write an equation for this reaction.
Using the Boltzmann distribution shown, explain why a catalyst raises the rate of this reaction.
Draw a three-dimensional diagram to show the shape of an ammonia molecule. Name the shape and state the bond angle.
Using Le Chatelier’s Principle and reaction kinetics, state and explain one benefit and one drawback of using a higher temperature.
State the equilibrium constant expression, $K_p$, for making ammonia from nitrogen and hydrogen in the Haber process.
A vessel initially contains $2.00$ moles of nitrogen and $3.00$ moles of hydrogen and is allowed to reach equilibrium. When equilibrium is reached, the pressure is $2.00 \times 10^7\ \text{Pa}$ and the mixture has $1.60$ moles of ammonia. Calculate $K_p$. Include the units.