The symbol equation for the industrial production of ammonia is shown. (a) Name this industrial process. .......................................................................................................................................... (b) State the meaning of $$$\Delta H$$$. .......................................................................................................................................... (c) State the typical conditions and name the catalyst used in the industrial production of ammonia. temperature and units .................................... pressure and units ......................................... catalyst used .................................................. (d) State two methods of increasing the rate of this reaction. 1 ............................................................................................................................................. 2 ............................................................................................................................................. The symbol equation for the reaction can be represented as shown in Fig. 3.1. Fig. 3.1 Table 3.1 shows some bond energies. Use the bond energies in Table 3.1 and $$$\Delta H$$$ to calculate the bond energy of an $$$\mathrm{N}-\mathrm{H}$$$ bond, in $$$\mathrm{kJ} / \mathrm{mol}$$$. Use the following steps. - Calculate the energy needed to break bonds in the reactants. .......................... kJ - Calculate the energy released when bonds form in the products. .......................... kJ - Calculate the energy of an $$$\mathrm{N}-\mathrm{H}$$$ bond. .......................... $$$\mathrm{kJ} / \mathrm{mol}$$$

Chemistry

IGCSE&ALevel

CAIE

Exam No：0620_s24_qp_42 Year：2024 Question No：3(e)

Answer:

Knowledge points:

4.1.1. Define electrolysis as the decomposition of an ionic compound, when molten or in aqueous solution, by the passage of an electric current

4.1.10. Predict the identity of the products at each electrode for the electrolysis of a halide compound in dilute or concentrated aqueous solution

4.1.11. Construct ionic half-equations for reactions at the anode (to show oxidation) and at the cathode (to show reduction)

4.1.2.1. the anode as the positive electrode

4.1.2.2. the cathode as the negative electrode

4.1.2.3. the electrolyte as the molten or aqueous substance that undergoes electrolysis

4.1.3.1. molten lead(II) bromide

4.1.3.2. concentrated aqueous sodium chloride

4.1.3.3. dilute sulfuric acid using inert electrodes made of platinum or carbon / graphite

4.1.4. State that metals or hydrogen are formed at the cathode and that non-metals (other than hydrogen) are formed at the anode

4.1.5. Predict the identity of the products at each electrode for the electrolysis of a binary compound in the molten state

4.1.6. State that metal objects are electroplated to improve their appearance and resistance to corrosion

4.1.7. Describe how metals are electroplated

4.1.8.1. the movement of electrons in the external circuit

4.1.8.2. the loss or gain of electrons at the electrodes

4.1.8.3. the movement of ions in the electrolyte

4.1.9. Identify the products formed at the electrodes and describe the observations made during the electrolysis of aqueous copper(II) sulfate using inert carbon / graphite electrodes and when using copper electrodes

5.1.1. State that an exothermic reaction transfers thermal energy to the surroundings leading to an increase in the temperature of the surroundings

5.1.2. State that an endothermic reaction takes in thermal energy from the surroundings leading to a decrease in the temperature of the surroundings

5.1.3. Interpret reaction pathway diagrams showing exothermic and endothermic reactions

5.1.4. State that the transfer of thermal energy during a reaction is called the enthalpy change

5.1.5. Define activation energy

5.1.6.1. reactants

5.1.6.2. products

5.1.6.3. enthalpy change of the reaction

5.1.6.4. activation energy

5.1.7. State that bond breaking is an endothermic process and bond making is an exothermic process and explain the enthalpy change of a reaction in terms of bond breaking and bond making

Answer:

Knowledge points:

Solution:

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