What is the molarity of ZnCl2 that forms when 30.0g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL . (please explain step by step I have no clue!)
Zn(s) + CuCl2(aq) --> ZnCl2(aq)+ Cu(s)
the answer is approximately 1.6098 M
From the equation 1 mole of Zn(s) gives 1 mole of ZnCl2(aq)
Number of moles of Zn is mass/molar mass of Zn
30.0 g /65.39 g mole^-1
=0.4588 mole
so 0.4588 mole ZnCl2 is formed (because 1 mole of Zn(s) gives 1 mole of ZnCl2(aq))
which is in 285 ml final volume
molarity is moles/volume (in L)
molarity =
0.4588 mole/0.285 L
l.64
Oh boy, chemistry! Let's break it down step by step, but keep it fun, shall we?
Step 1: Calculate the molar mass of Zn.
Zn has an atomic mass of 65.38 g/mol. So, 30.0g of Zn is equal to 30.0g / 65.38 g/mol = 0.459 mol of Zn. Good job!
Step 2: Calculate the number of moles of ZnCl2.
According to the balanced equation, 1 mole of Zn reacts to form 1 mole of ZnCl2. Since we have 0.459 mol of Zn, we will have the same amount of moles for ZnCl2. Easy peasy!
Step 3: Calculate the molarity of ZnCl2.
Molarity is defined as the number of moles of solute divided by the volume of solution in liters. We're given the final volume of 285 mL, so we need to convert it to liters. There are 1000 mL in a liter, so 285 mL = 0.285 L.
Now, we can calculate the molarity of ZnCl2. Molarity (M) = moles of solute / volume of solution in liters. In this case, it will be 0.459 mol / 0.285 L = 1.609 M.
So, the molarity of ZnCl2 is approximately 1.609 M. Ta-da!
Now that we've solved the problem, I hope your confusion has diminished faster than a clown car pulling away!
To calculate the molarity of ZnCl2 that forms when 30.0g of zinc reacts with CuCl2 according to the given reaction, we need to follow these steps:
Step 1: Determine the moles of zinc.
Given the mass of zinc (30.0g) and the molar mass of zinc (65.38 g/mol), we can calculate the moles of zinc using the formula:
moles = mass / molar mass
moles of zinc = 30.0g / 65.38 g/mol
Step 2: Determine the stoichiometry of the reaction.
From the balanced chemical equation, we can see that 1 mole of Zn reacts with 1 mole of CuCl2 to produce 1 mole of ZnCl2. This means that the moles of ZnCl2 formed will be equal to the moles of zinc used.
Step 3: Determine the volume in liters.
Given that the final volume is 285 mL, we need to convert it to liters. We can use the conversion factor:
1 L = 1000 mL
285 mL x (1 L / 1000 mL) = 0.285 L
Step 4: Calculate the molarity.
Molarity is defined as the moles of solute divided by the volume of the solution in liters. In this case, the solute is ZnCl2, and we have already determined the moles of ZnCl2 formed (which is equal to the moles of zinc used). So, we can use the formula:
molarity = moles of solute / volume of solution (in liters)
molarity = moles of ZnCl2 / 0.285 L
Substitute the value of moles of ZnCl2 we calculated earlier into the formula to find the molarity.