Question

A chemist used 6.5 moles of water in this reaction. How many grams of water were used?

please go into detail as to why that is the answer PLSSS

Answer 1

`\boxed {\boxed {\sf 120 \ or \ 117 \ grams \ H_2O \ depending \ on \ significant \ figures }}`

Step-by-step explanation:

We want to convert from moles of water to grams of water.

First, find the molar mass of water (H₂O) Look on the Periodic Table for the masses of hydrogen and oxygen.

• Hydrogen (H): 1.008 g/mol
• Oxygen (O): 15.999 g/mol

Next, add up the number of each element in water. The subscript of 2 comes after the H, so there are 2 moles of hydrogen.

• 2 Hydrogen: (1.008 g/mol*2) = 2.016 g/mol

Finally, add the molar mass of 2 hydrogen and 1 oxygen.

• 2.016 g/mol (2 Hydrogen) + 15.999 g/mol (1 oxygen)= 18.015 g/mol

Next, find the grams in 6.5 moles.

Use the molar mass we just found as a ratio.

`molar \ mass \ ratio: (18.015 \ g \ H_2O)/(1 \ mol \ H_2O)`

We want to find the grams in 6.5 moles. We can multiply the ratio above by 6.5

`6.5 \ mol \ H_2O * (18.015 \ g \ H_2O)/(1 \ mol \ H_2O)`

Multiply. Note that the moles of H₂O will cancel each other out.

`6.5 * (18.015 \ g \ H_2O)/(1)`

`6.5 * {18.015 \ g \ H_2O}`

`117.0975 \ g \ H_2O`

If we want to round to the technically correct significant figures, it would be 2 sig figs. The original measurement, 6.5, has 2 (6 and 5).

`\approx 120 \ g \ H_2O`