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Andreas93 [3]
3 years ago
15

Iron(II) sulfide has a molar mass of 87.91 g/mol. 50 grams of

Chemistry
2 answers:
dimaraw [331]3 years ago
7 0

Answer:

true

Explanation:

Temka [501]3 years ago
7 0

Answer:

\boxed {\boxed {\sf False}}

Explanation:

We want to know if 50 grams of iron (II) sulfide contains 3.011 * 10²³ molecules.  Let's calculated and check.

<h3>1. Convert Grams to Moles</h3>

We know there are 50 grams of iron (II) sulfide or FeS If we want to convert from grams to moles, we use the molar mass (mass per 1 mole). This is given to us and it is 87.91 grams per mole for this substance. Let's create a ratio.

\frac {87.91 \ g \ FeS}{ 1 \ mol \ FeS}

We want to convert 50 grams of FeS to moles, so we multiply by this value.

50 \ g \ FeS *\frac {87.91 \ g \ FeS}{ 1 \ mol \ FeS}

Flip the ratio so the grams of FeS cancel.

50 \ g \ FeS *\frac {1 \ mol \ FeS}{ 87.91 \ g \ FeS}

50*\frac {1 \ mol \ FeS}{ 87.91}

\frac {50}{ 87.91} \ mol \ FeS

0.5687635081 \ mol \ FeS

<h3>2. Convert Moles to Molecules</h3>

1 mole of any substance contains the same number of particles (atoms, molecules, formula units, etc.). This is Avogadro's Number or 6.022 *10²³. In this case, the particles are molecules of FeS. Create another ratio.

\frac {6.022  *10^{23} \ molecules \ FeS}{ 1 \ mol \ FeS}

We want to convert 0.5687635081 moles of FeS to molecules, so we multiply by this value.

0.5687635081 \ mol \ FeS*\frac {6.022  *10^{23} \ molecules \ FeS}{ 1 \ mol \ FeS}

The units of moles of FeS cancel.

0.5687635081 *\frac {6.022  *10^{23} \ molecules \ FeS}{ 1 }

0.5687635081 *{6.022  *10^{23} \ molecules \ FeS}

3.42509385*10^{23} \ molecules \ FeS

If we round to the thousandth place, the 0 in the tenth thousandth place tells us to leave the 5.

3.425*10^{23} \ molecules \ FeS

50 grams of iron (II) sulfide is approximately 3.425 * 10²³ molecules, not 3.011 *10²³ so the statement is false.

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