What preperation produces a 2.0 Mole solution of C6H12O6?

a) 90.0 grams of C6H12O6 dissolved in 500.0 mL of solution
b) 180.0 grams of C6H12O6 dissolved in 1000mL of solution
c) 90 Grams of C6H12O6 dissolved in 1000mL of solution
D) 180.0 Grams of C6H12O6 dissolved in 500.0mL of solution

To calculate the molarity (M) of a solution, you need to know the moles of solute (C6H12O6) and the volume of the solution.

Given options:
a) 90.0 grams of C6H12O6 dissolved in 500.0 mL of solution
b) 180.0 grams of C6H12O6 dissolved in 1000mL of solution
c) 90 Grams of C6H12O6 dissolved in 1000mL of solution
d) 180.0 Grams of C6H12O6 dissolved in 500.0mL of solution

To determine the correct option, we need to calculate the moles of C6H12O6 in each case using its molar mass, which is 180.16 g/mol.

Let's calculate the moles for each option:

a) Moles = mass / molar mass
Moles = 90.0 g / 180.16 g/mol
Moles ≈ 0.4999 mol

b) Moles = mass / molar mass
Moles = 180.0 g / 180.16 g/mol
Moles ≈ 0.9998 mol

c) Moles = mass / molar mass
Moles = 90 g / 180.16 g/mol
Moles ≈ 0.4999 mol

d) Moles = mass / molar mass
Moles = 180.0 g / 180.16 g/mol
Moles ≈ 0.9998 mol

Now, let's calculate the molarity (M) for each option using the formula:

Molarity (M) = moles / volume

a) Molarity = 0.4999 mol / 0.500 L
Molarity = 0.9998 M

b) Molarity = 0.9998 mol / 1.000 L
Molarity = 0.9998 M

c) Molarity = 0.4999 mol / 1.000 L
Molarity = 0.4999 M

d) Molarity = 0.9998 mol / 0.500 L
Molarity = 1.9996 M

Based on the calculations, the option that produces a 2.0 Mole solution of C6H12O6 is option d) 180.0 grams of C6H12O6 dissolved in 500.0 mL of solution.

To determine the correct answer, we need to calculate the number of moles of C6H12O6 in each option and see if it matches the desired 2.0 moles.

First, we need to convert grams of C6H12O6 to moles using the molar mass of C6H12O6. The molar mass of C6H12O6 is:
6 * 12.01 g/mol (Carbon) + 12 * 1.01 g/mol (Hydrogen) + 6 * 16.00 g/mol (Oxygen) = 180.18 g/mol

Now let's calculate the number of moles for each option:

a) 90.0 grams of C6H12O6 dissolved in 500.0 mL of solution:
Number of moles = (90.0 g) / (180.18 g/mol) = 0.499 moles (approximately)

b) 180.0 grams of C6H12O6 dissolved in 1000 mL of solution:
Number of moles = (180.0 g) / (180.18 g/mol) = 0.998 moles (approximately)

c) 90 grams of C6H12O6 dissolved in 1000 mL of solution:
Number of moles = (90.0 g) / (180.18 g/mol) = 0.499 moles (approximately)

D) 180.0 grams of C6H12O6 dissolved in 500.0 mL of solution:
Number of moles = (180.0 g) / (180.18 g/mol) = 0.998 moles (approximately)

Comparing the calculated number of moles with the desired 2.0 moles, we can see that options b and d have the closest number of moles (approximately 0.998 moles). Therefore, the correct answer is option b) 180.0 grams of C6H12O6 dissolved in 1000 mL of solution.

I don't think you intended to write this question. The correct answer for THIS question is "none of these." I think you meant "which of the following produces a 2 MOLAR solution.

mols = grams/molar mass, then
M = mols/L soln.
Check each one and see which is 2.0 M.