Questions: Consider the following balanced reaction: 3 SCl2(l) + 4 NaF(s) -> SF4(g) + S2 Cl2(l) + 4 NaCl(s) How many grams of sodium fluoride are needed to form 485 g of sulfur tetrafluoride?

Consider the following balanced reaction:
3 SCl2(l) + 4 NaF(s) -> SF4(g) + S2 Cl2(l) + 4 NaCl(s)

How many grams of sodium fluoride are needed to form 485 g of sulfur tetrafluoride?

Transcript text: Consider the following balanced reaction: \[ 3 \mathrm{SCl}_{2}(l)+4 \mathrm{NaF}(s) \longrightarrow \mathrm{SF}_{4}(g)+\mathrm{S}_{2} \mathrm{Cl}_{2}(l)+4 \mathrm{NaCl}(s) \] How many grams of sodium fluoride are needed to form 485 g of sulfur tetrafluoride?

Solution

Solution Steps

Step 1: Determine the molar masses of the relevant compounds

First, we need to find the molar masses of sodium fluoride (NaF) and sulfur tetrafluoride (SF\(_4\)).

Molar mass of NaF: \[ \text{Na} = 22.99 \, \text{g/mol}, \quad \text{F} = 18.998 \, \text{g/mol} \] \[ \text{Molar mass of NaF} = 22.99 + 18.998 = 41.988 \, \text{g/mol} \]
Molar mass of SF\(_4\): \[ \text{S} = 32.06 \, \text{g/mol}, \quad \text{F} = 18.998 \, \text{g/mol} \] \[ \text{Molar mass of SF}_4 = 32.06 + 4 \times 18.998 = 108.052 \, \text{g/mol} \]

Step 2: Calculate the moles of SF\(_4\) produced

Next, we convert the given mass of SF\(_4\) to moles.

\[ \text{Moles of SF}_4 = \frac{485 \, \text{g}}{108.052 \, \text{g/mol}} = 4.488 \, \text{mol} \]

Step 3: Use stoichiometry to find the moles of NaF needed

From the balanced chemical equation, we see that 1 mole of SF\(_4\) requires 4 moles of NaF.

\[ \text{Moles of NaF} = 4 \times \text{Moles of SF}_4 = 4 \times 4.488 = 17.952 \, \text{mol} \]

Step 4: Convert moles of NaF to grams

Finally, we convert the moles of NaF to grams.

\[ \text{Mass of NaF} = 17.952 \, \text{mol} \times 41.988 \, \text{g/mol} = 753.9 \, \text{g} \]