### Hydrogen Gas: Industrial Production and Reactions#### Introduction:Hydrogen gas is an essential industrial molecule used extensively in the production of various compounds, such as in the Haber-Bosch process for ammonia production.#### Reactions:One of the primary industrial methods for producing hydrogen gas (H₂) involves the exothermic reaction of methane (CH₄) and water (H₂O). #### Chemical Equation:\[ \text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow 3 \text{H}_2(g) + \text{CO}(g) \]This reaction releases energy with an enthalpy change (ΔH) of 206 kJ per mole.#### Tasks:a. **Potential Energy Diagram**: Using the provided chemical reaction, draw a potential energy diagram. The diagram should show the energy changes during the reaction:1. The y-axis represents potential energy.2. The x-axis represents the progress of the reaction from reactants to products.3. Indicate the energy of the reactants (CH₄ and H₂O) and the products (H₂ and CO).4. Highlight the difference in energy, showing that the reaction is exothermic.b. **Effect of a Catalyst**:Draw a second line on the same diagram to represent the reaction with a catalyst. The catalyst lowers the activation energy but does not change the reactants' or products' potential energies.#### Explanation:- A potential energy diagram visually represents the energy levels of reactants and products during a chemical reaction.- In an exothermic reaction, the potential energy of the products is lower than that of the reactants, resulting in energy release.- When a catalyst is present, it reduces the activation energy required for the reaction without altering the initial and final energy states, thereby increasing the reaction rate.By understanding these diagrams, students can better comprehend the energy dynamics involved in chemical reactions, particularly those industrially relevant like the production of hydrogen gas.

Potential energy diagram is a plot of energy along the vertical axis and reaction coordinate along…

10. Hydrogen gas is an important industrial molecule used in the production of many other compounds (for example the Haber-Bosch production of ammonia). The following exothermic reactions of methane and water is used industrially to produce H₂ gas. CH₂(g) + H₂O (g) 3 H₂(g) + CO (g) AH=206 kJ/mol a. Using the axes below, draw a potential energy diagram for the production of hydrogen gas using the above reaction. b. Draw a second line representing the same reaction with a catalyst.

10. Hydrogen gas is an important industrial molecule used in the production of many other compounds (for example the Haber-Bosch production of ammonia). The following exothermic reactions of methane and water is used industrially to produce H₂ gas. CH₂(g) + H₂O (g) 3 H₂(g) + CO (g) AH=206 kJ/mol a. Using the axes below, draw a potential energy diagram for the production of hydrogen gas using the above reaction. b. Draw a second line representing the same reaction with a catalyst.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which of the following represents an endothermic reaction? CH4 (g) + 202 (g) → CO2 (g) + 2H2O (g) + 890 kJ 2C2H6 (g) + 702 (g) → 4CO2 (g) + 6H20(g) + 3120 kJ 2SO2 (g) → 25 (s) + 202 (g) + 376KJ 2H20 (g) + 572 kJ → 2H2 (g) + O2 (g)
A chemist measures the enthalpy change ΔH during the following reaction: 2Al(OH)3(s)→Al2O3(s)+ 3H2O(l) ΔH=41.kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔH Al2O3(s) + 3H2O(l) → 2Al(OH)3(s) kJ 3Al2O3(s) + 9H2O(l) → 6Al(OH)3(s) kJ 4Al(OH)3(s)+2Al2O3(s) + 6H2O(l) kJ
Calcium hydroxide is prepared by adding calcium oxide to water: CaO (s) + H2O (l) → Ca(OH)2 (s) Calculate the enthalpy change (ΔH) for this reaction considering the following experiment. A 10.0 g sample of CaO (s) {MM = 56.08 g/mol} is added to 1.00 liter of water in a calorimeter with a total heat capacity of 4.37 kJ K-1 and the temperature increases by 2.70 K.
3. Calcium sulfate is a byproduct of some types of oil extraction. Some companies process the calcium sulfate by extracting sulfur from it. The first step in this sequence is CaSO4(s) + CO(9) CaO(s) + SO2(g) + CO2(g) If you have 36kg of calcium sulfate to process, how much energy will be transferred? (Give the amount, and clearly state whether the energy is absorbed or released.)
Which of the following represents an endothermic reaction? O CH4 (g) + 202 (g) → CO2 (g) + 2H2O (g) + 890 kJ 2S02 (g) 25 (s) + 20, (g) + 376kJ O 2C2H6 (g) + 702 (g) → 4CO2 (g) + 6H2O(g) + 3120 kJ 2H20 (g) + 572 kJ → 2H2 (g) + O2 (g)
Many manufactures produce hydrogen gas from methane gas, as in the reaction below. This reaction is endothermic, with DHrxn = 206.1 kJ. How much heat energy is required to produce 2.50 kg of hydrogen gas? CH4 (g) + H2O (g) = CO (g) + 3H2 (g)
Titanium reacts with iodine to form titanium(III) iodide, emitting heat:2 Ti(s) + 3 I2(g) ---------> 2 TiI3(s) ∆H°rxn = -839 kJDetermine the masses of titanium and iodine that react if 1.55 x 103 kJ of heat is emitted by the reaction.
When CO(g) reacts with NO(g) according to the following reaction, 373 kJ of energy are evolved for each mole of CO(g) that reacts. Complete the following thermochemical equation. 2CO(g) + 2NO(g)- →2CO₂(g) + N₂(g) ΔΗ = kJ
The combustion of 0.1587 g benzoic acid increases the temperature of a bomb calorimeter by 2.57°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2140-g sample of vanillin (CHO3) is then burned in the same calorimeter, and the temperature increases by 3.25°C. What is the energy of combustion per gram of vanillin? Energy= kJ/g %3D Per mole of vanillin? Energy = kJ/mol %3D
Part 2 The Haber process produces ammonia (NH3) for the chemical industry from nitrogen (N₂) and hydrogen (H₂) as shown in the chemical equation below. This is a reversible reaction. N2 (8) + 3H2(g) → 2NH3 (8) AH = -92 kJ mol-¹ (exothermic) The following questions relate to the effect of changing factors that influence the direction of the above reaction, according to Le Chatelier's principle. For each change in factor (i - iv) listed in the Table, you need to: state the direction of equilibrium, give a reason for your choice, identify if the amount of ammonia produced will increase or decrease. Factor Decrease in concentration of N₂ i) ii) Increase in pressure iii) Increase in temperature iv) A catalyst is added Direction (shift) of equilibrium Scientific explanation for stated direction of equilibrium. Amount of NH3 Increases / decreases Part 3 During this reaction, compromises are made to speed up and maximise the production of ammonia. i) ii) Suggest why a moderate amount of…
Determine the standard enthalpy (ΔH) for this reaction and explain the cooling effect that is experienced when methanol is accidentally dropped on the skin. The standard enthalpy of formation for CH3OH(l) is -239.1 kJ/mol and for CH3OH(g) is -189.83 kJ/mol. CH3OH(l) → CH3OH(g)
Nitrogen oxide (NO) has been found to be a key component in many biological processes. It also can react with oxygen to give the brown gas NO2. When one mole of NO reacts with oxygen, 57.0 kJ of heat are evolved. How many grams of nitrogen oxide must react with an excess of oxygen to liberate 20 kJ of heat? NO(g) + ½O2(g) → NO2(g) ΔH = –57.0 kJ ___________ g