Question

How many liters are in 4.65 E 23 molecules of F2?

Answer 1

I need more points sorry

Answer 2

`\boxed {\boxed {\sf 17.3 \ L \ F_2}}`

Step-by-step explanation:

First, we must convert molecules to moles.

We use Avogadro's Number: 6.022*10²³. This number tells us the amount of particles (atoms, molecules, etc.) in 1 mole of a substance. In this case, it is molecules of F₂

`( 6.022*10^(23) \ molecules \ F_2)/(1 \ mol \ F_2)`

Multiply by the given number of molecules.

`4.65 *10^(23) \ molecules \ F_2*( 6.022*10^(23) \ molecules \ F_2)/(1 \ mol \ F_2)`

Flip the fraction so the molecules of fluorine cancel.

`4.65 *10^(23) \ molecules \ F_2*(1 \ mol \ F_2 )/(6.022*10^(23) \ molecules \ F_2)`

`4.65 *10^(23) *(1 \ mol \ F_2 )/(6.022*10^(23) )`

`(4.65 *10^(23) \ mol \ F_2 )/(6.022*10^(23) )=0.7721687147 \ mol \ F_2`

Next, convert the moles to liters. Assuming this is at STP (standard temperature and pressure), there are 22.4 liters in 1 mole of any gas.

`\frac {22.4 \ L \ F_2} {1 \ mol \ F_2}`

Multiply by the number of moles we calculated.

`0.7721687147 \ mol \ F_2*\frac {22.4 \ L \ F_2} {1 \ mol \ F_2}`

The moles of fluorine cancel.

`0.7721687147 *\frac {22.4 \ L \ F_2} {1 }`

`0.7721687147 *\ {22.4 \ L \ F_2} =17.29657921 \ L \ F_2`

The original measurement has 3 significant figures (4, 6, and 5), so our answer must have the same. For the number we calculated, that is the tenth place. The 9 in the hundredth place tells us to round the 2 up to a 3.

`17.3 \ L \ F_2`

There are approximately 17.3 liters of fluorine.