Question

What is the mass (in grams) of 8.45 x 1023 molecules of dextrose: C6H12O6 (Mw. 180.16 g/mol)?

Answer 1

The mass of 8.45 x 10^23 molecules of dextrose is calculated by dividing the number of molecules by Avogadro's number to find the moles, and then multiplying by the molar mass, resulting in 252.74 grams.

Step-by-step explanation:

The question asks about calculating the mass of 8.45 x 1023 molecules of dextrose (C6H12O6). To find the mass in grams, we need to know how many moles of dextrose these molecules correspond to and use the molar mass of C6H12O6.

First, we establish the number of moles of dextrose by utilizing Avogadro's number (6.022 x 1023 molecules/mol). This is done by dividing the given number of molecules (8.45 x 1023) by Avogadro's number:

1. Number of moles = 8.45 x 1023 molecules / 6.022 x 1023 molecules/mol = 1.403 moles.
2. Next, we multiply the number of moles by the molar mass of dextrose to find the mass:
3. Mass = 1.403 moles x 180.16 g/mol = 252.74 g.

Therefore, the mass of 8.45 x 1023 molecules of dextrose is 252.74 grams.

Answer 2

The mass (in grams) of 8.45 x 10^23 molecules of dextrose is 252.798g Working: Mw. dextrose is 180.16 g/mol therefore 180.16 grams dextrose = 1 mole therefore 180.16 grams dextrose= 6.022x10^23 molecules (Avogadro's number) We have 8.45 x 10^23 molecules of dextrose. Therefore, (180.16 divided by 6.022x10^23) times 8.45x10^23 gives the mass (in grams) of 8.45 x 10^23 molecules of dextrose; 252.798.