question 1 (Hand in at the start of the experiment) SectionGr Experiment 3: Prel

Question

question 1

(Hand in at the start of the experiment) SectionGr Experiment 3: Prelab Worksheet Grade Date Name Record all values with the correct number of significant figures and units Place all answers on the line next to the question Show calculations for any numerical answers See any 114 TA in the help office before your prelab is due if you have any questions Your answer must be completely correct to get any credit for the answer, no partial credit. 1. Why do you use an excess of iron nitrate when making the standard curve for this experiment? 2. Which solutions do you use to make your Beer's Law plot, the standard solutions, the equilibrium solutions or both? 3. What is the final concentration of Fe in a solution if you add 2.5 ml of 3.0M Fe(NO)s and 3.2ml of water in a test tube? Answer the next two questions based on the following reaction. H2(g) + 1/2S2(g) = H2S(g) 4. Write Ke for the given reaction above. 5. Write the expression for Ke for the production of 4 moles of H2(9). (Hint: How does chemical equatic change?) 59

Explanation / Answer

Reaction with iron nitrate

1. Excess iron nitrate is used for the reaction while drawing the data for calibration curve. This is due to the fact that, excess iron nitrate would push the equilibrium towards the right handside by reacting with all of the SCN- reagent, that is towards the product. The limiting reactant in this case is SCN-. All of SCN- forms the complex and the concentration of SCN- is equal to the concentration of the complex ion product formed in the reaction.

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