A solution is prepared by mixing 5.00 mL of 0.00100M iodine, 10 mL of 0.500M HCl, and 10 mL of 2.00M acetone with 15 mL of water A) Calculate the concentration of iodine in the final solution, before any reaction occurs. B) Calculate the concentration of acetone in the final solution, before any reaction occurs.
A solution is prepared by mixing 5.00 mL of 0.00100M iodine, 10 mL of 0.500M HCl, and 10 mL of 2.00M acetone with 15 mL of water
A) Calculate the concentration of iodine in the final solution, before any reaction occurs.
B) Calculate the concentration of acetone in the final solution, before any reaction occurs.
C) When the reaction is complete, the iodine will be used up. What will be the concentration of acetone in the solution afterthe reaction is complete? (see the balanced equation;one mole of acetonereacts with one mole of iodine). What percentage of the acetone has been used up when the reaction is complete
D) The rate of the reaction can be expressed as −Δ[I2]/Δt. If the reaction given above requires 63 seconds for completion, what isthe rate of the reaction? Include units.
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