Chemistry - Chemistry
Draw an energy diagram for an endothermic reaction without a catalyst (use a solid line) and with a catalyst (use a dotted line). Label all parts of the diagram. Explain what a catalyst is and how a catalyst influences the rate of a reaction.Graded Assignment SCI303B: Chemistry | Unit 5 | Lesson 8: Mid-Unit Test Name: Lily Johnson Date: February 1, 2021 Graded Assignment Mid-Unit Test, Part 2 Answer the questions below. When you have finished, submit this assignment to your teacher by the due date for full credit. (8 points) Score Click or tap here to enter text. This energy diagram is for the thermal decomposition of solid mercury (II) oxide (also known as mercuric oxide) into liquid mercury and oxygen gas. A graph. The x-axis is labeled Reaction pathway. The y-axis is labeled Energy. A dashed horizontal line labeled Reactants is plotted at about one-fifth across the y-axis. A dashed horizontal line labeled Activated complex is plotted near the top of the y-axis. A line labeled Products is plotted on the graph. Products starts at the origin of Reactants, extends horizontally to the right, curves upward to the right with downward opening until Activated complex, slightly curves downward to the right, and extends horizontally to the right. The distance between Reactans and Activated complex is labeled (a). Write a balanced equation for the reaction. Explain what feature is shown by the arrow labeled (a). Using chemical symbols and dashed lines (this can be done with type), draw what the activated complex or transition state might look like. Is this reaction exothermic or endothermic? Explain. Answer: Question: The Equation For The Decomposition Of Mercury (II) Oxide 2HgO (s) --> 2Hg (s) + O2 (g) Change In H = 181.6 KJ If 167.0 KJ Of Heat Energy Is Absorbed By This Reaction, Will The Reaction Produce More Mercury (II) Oxide Or Consume The Mercury (II) Oxide? Balanced equation: 2 HgO (s) - > 2 Hg (l) + O2 (g) Reaction needs energy because energy of products is higher that energy of Reactants, that how you find out is reaction exo- or endothermic First off write out the reaction equation given, HgO(g) -> O2(l) + Hg(g) You will need to balance it. The transition state for a reaction is the point where the reactant is structurally between products and reactant (this state exists for only an instant). Dashed lines in a chemical structure represent partial covalent bonds, essentially in a transition state they represent the bonds that are being broken and the new bonds being formed. For example: The reaction of CH3I + NaOH -> CH3OH + NaI Attached is the transition state drawing, the brakets and double dagger symbol at the top is just standard notation for a transition state The structure of O2 and HgO is simply O=O and Hg=O respectively. 1) 2HgO ------> 2Hg + O2 2) (a) Arrow show the difference between the energy of activated complex and energy of reactants. 3) .........Sorry here is confusion 4) It is endothermic reaction, because Graph show that the energy of product is greater than reactants, which mean reactants got energy by heating during the reaction, due to whic energy of products is high, so reaction is endothermic. (8 points) Score Click or tap here t
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