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!
0.038 mol FeCl2 x (1 mol K2Cr2O7/6 mol FeCl2) = mols K2Cr2O7.
Then M = mols/L so
L = mols/M =
Then multiply by 1000 to convert to mL.
Well, chemistry can be quite confusing at times, but don't worry, I'm here to help!
First, let's determine the number of moles of FeCl2 you have:
0.038 moles of FeCl2.
Now, we need to use the balanced equation to find the stoichiometric ratio between FeCl2 and K2Cr2O7. According to the equation:
6 FeCl2(aq) + K2Cr2O7(aq) + 14 HCl(aq) ==>
6 FeCl3(aq) + 2 CrCl3(aq) + 2 KCl(aq) + 7 H2O(l)
We can see that 1 mole of FeCl2 reacts with 1/6 mole of K2Cr2O7. Therefore, the number of moles of K2Cr2O7 required can be calculated as:
0.038 moles of FeCl2 * (1/6) moles of K2Cr2O7/1 mole of FeCl2 = 0.00633 moles of K2Cr2O7.
Finally, we can use the equation Molarity = Mole/Volume to find the volume of the K2Cr2O7 solution:
Molarity = 0.0750 M.
Moles = 0.00633 moles of K2Cr2O7 (which we calculated earlier).
0.0750 M = 0.00633 moles of K2Cr2O7/Volume
Volume = 0.00633 moles of K2Cr2O7 / 0.0750 M = 0.0844 L.
Since we want the answer in milliliters, we multiply 0.0844 L by 1000:
Volume = 0.0844 L * 1000 mL/L = 84.4 mL.
So, you need approximately 84.4 milliliters of the 0.0750 M K2Cr2O7 solution to react with 0.038 moles of FeCl2.
I hope this helps, and remember, when in doubt, just keep calm and chemistry on!
To find the volume of 0.0750 M K2Cr2O7(aq) needed to react with 0.038 mol of FeCl2(aq), we can use the balanced equation and the stoichiometry of the reaction.
From the balanced equation:
6 mol of FeCl2(aq) reacts with 1 mol of K2Cr2O7(aq)
The number of moles of K2Cr2O7(aq) can be calculated by the molar ratio:
0.038 mol FeCl2(aq) * (1 mol K2Cr2O7(aq) / 6 mol FeCl2(aq)) = 0.00633 mol K2Cr2O7(aq)
Now we can use the equation Molarity = Mole/Volume:
0.0750 M = 0.00633 mol / Volume
To isolate the volume, we rearrange the equation:
Volume = 0.00633 mol / 0.0750 M
Volume = 0.0844 L
To convert the volume from liters to milliliters, multiply by 1000:
Volume = 0.0844 L * 1000 = 84.4 mL
Therefore, 84.4 mL of 0.0750 M K2Cr2O7(aq) will react with 0.038 mol of FeCl2(aq).
To solve this question, we can use the equation you mentioned: Molarity = Mole/Volume. However, let's break it down step by step to ensure we get the correct answer.
First, we need to determine the number of moles of FeCl2(aq) that react with K2Cr2O7(aq). According to the balanced chemical equation, the stoichiometric ratio between FeCl2(aq) and K2Cr2O7(aq) is 6:1. Therefore, for every 6 moles of FeCl2(aq), 1 mole of K2Cr2O7(aq) is consumed.
In this particular problem, you are given that there are 0.038 moles of FeCl2(aq). To calculate the moles of K2Cr2O7(aq), we can use the stoichiometric ratio:
(0.038 mol FeCl2(aq)) x (1 mol K2Cr2O7(aq)/6 mol FeCl2(aq)) = 0.00633 mol K2Cr2O7(aq)
Now, we know the amount of K2Cr2O7(aq) in moles. The next step is to find the volume of the K2Cr2O7(aq) solution.
To do this, we can rearrange the equation: Molarity = Mole/Volume to solve for Volume:
Volume = Mole/Molarity
Given that the molarity is 0.0750 M for K2Cr2O7(aq) and you want to find the volume in milliliters, we can plug in the values:
Volume = (0.00633 mol)/(0.0750 mol/L) = 0.0844 L
Next, we convert this volume to milliliters:
0.0844 L x (1000 mL/1 L) = 84.4 mL
Therefore, 84.4 mL of the 0.0750 M K2Cr2O7(aq) solution will react with 0.038 mol of FeCl2(aq).