6 FeCl2(aq) + K2Cr2O7(aq) + 14 HCl(aq) ==>
6 FeCl3(aq) + 2 CrCl3(aq) + 2 KCl(aq) + 7 H2O(l)
How many milliliters of 0.0750 M K2Cr2O7(aq) will react with 0.038 mol of FeCl2(aq)?
I used the equation Molarity=Mole/Volume
and divided my answer by 1000 to get milliliters. I'm still getting the answer wrong for some reason. Please help! Thank you!
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To answer this question, we need to use stoichiometry to determine the number of moles of K2Cr2O7 that will react with the given amount of FeCl2. Here's how you can calculate it step by step:
1. Write the balanced equation for the reaction:
6 FeCl2(aq) + K2Cr2O7(aq) + 14 HCl(aq) → 6 FeCl3(aq) + 2 CrCl3(aq) + 2 KCl(aq) + 7 H2O(l)
2. From the equation, we can see that the stoichiometric ratio between FeCl2 and K2Cr2O7 is 6:1. This means that for every 6 moles of FeCl2, 1 mole of K2Cr2O7 will react.
3. Calculate the number of moles of K2Cr2O7 using the stoichiometry:
Given: Moles of FeCl2 = 0.038 mol
Moles of K2Cr2O7 = (0.038 mol FeCl2) * (1 mol K2Cr2O7 / 6 mol FeCl2)
= 0.00633 mol K2Cr2O7
4. Now, we need to convert the moles of K2Cr2O7 into milliliters of a 0.0750 M solution. To do this, we can use the equation:
Molarity = Moles / Volume
Rearranging the equation, we get:
Volume = Moles / Molarity
Volume = 0.00633 mol / 0.0750 M
= 0.0844 L
5. Finally, convert the volume from liters to milliliters by multiplying by 1000:
Volume (in milliliters) = 0.0844 L * 1000
= 84.4 mL
So, 84.4 milliliters of the 0.0750 M K2Cr2O7 solution will react with 0.038 moles of FeCl2.