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Topic 2: Managing Chemical Processes

7 dot points, in syllabus order. Each dot point has a focused answer, with exam-style questions and worked answers where available.

What does it mean for a reaction to reach dynamic equilibrium, and how does Kc describe it?

Describe dynamic equilibrium in closed systems and use the equilibrium constant expression Kc to relate equilibrium concentrations and reaction extent.

Dynamic equilibrium in closed systems, writing and interpreting the Kc expression, the ICE-table method, units and the temperature dependence of Kc, with fully worked SACE-style equilibrium-constant calculations.

9 min read →

How does a catalyst speed up a reaction without being consumed?

Explain how catalysts increase reaction rate by providing an alternative pathway with a lower activation energy, and represent this on an energy profile.

How catalysts lower activation energy by offering an alternative pathway, the Maxwell-Boltzmann explanation, homogeneous versus heterogeneous catalysis, energy profiles, and worked SACE-style rate and energy calculations.

8 min read →

How do industrial conditions for the Haber process balance reaction rate against equilibrium yield?

Explain how temperature, pressure and catalyst conditions in the Haber process are chosen to compromise between reaction rate and equilibrium yield.

How the Haber process balances rate against equilibrium yield: the effect of pressure, temperature and the iron catalyst, the compromise temperature, recycling, and worked SACE-style yield and economic-trade-off analysis.

9 min read →

How can chemical processes be designed to reduce waste and environmental impact?

Apply green chemistry principles, including atom economy, to evaluate the efficiency and sustainability of chemical processes.

The principles of green chemistry, the difference between atom economy and percentage yield, and how to evaluate a process for waste and sustainability, with fully worked SACE-style atom-economy and yield calculations.

8 min read →

How is the heat released or absorbed by a reaction measured and calculated?

Calculate enthalpy changes from calorimetry data using q = mcΔT, and interpret exothermic and endothermic reactions.

Using q = mcΔT to find heat transferred, converting to molar enthalpy change, the sign convention for exothermic and endothermic reactions, sources of heat loss, and fully worked SACE-style calorimetry calculations.

9 min read →

How does a system at equilibrium respond when conditions are changed?

Apply Le Chatelier's principle to predict the effect of changes in concentration, pressure and temperature on the position of equilibrium.

Predicting equilibrium shifts for changes in concentration, pressure, volume and temperature using Le Chatelier's principle, distinguishing position shifts from changes in Kc, with worked SACE-style prediction problems.

9 min read →

What factors control how fast a reaction proceeds, and why?

Use collision theory to explain the effect of concentration, surface area, temperature and pressure on reaction rate.

Collision theory, activation energy and the Maxwell-Boltzmann distribution explaining how concentration, surface area, temperature, pressure and catalysts change reaction rate, with worked SACE-style rate calculations.

8 min read →