QuestionHow many grams of fluorine ( $\mathrm{F}_{2}$ ) are needed for 3.25 moles of carbon tetrafluoride ( $\mathrm{CF}_{4}$ )? Molar mass of $\mathrm{F}_{2}$ is 38.00 g/mol. [?] g $\mathrm{F}_{2}$

Studdy Solution

STEP 1

Assumptions1. The chemical reaction is balanced and proceeds to completion. . The molar mass of $\mathrm{}_{}$ is $38.00 \mathrm{~g/mol}$ .
3. We want to find the mass of $\mathrm{}_{}$ required to produce $3.25$ moles of $\mathrm{CF}_{4}$ .

STEP 2

First, we need to understand the stoichiometry of the reaction. From the balanced chemical equation, we can see that one mole of carbon reacts with two moles of fluorine to produce one mole of carbon tetrafluoride.
$\mathrm{C}+2 \mathrm{~}_{2} \rightarrow \mathrm{CF}_{4}$

STEP 3

Now, we need to find out how many moles of $\mathrm{}_{2}$ are required to produce $3.25$ moles of $\mathrm{CF}_{}$ . From the stoichiometry of the reaction, we know that for every mole of $\mathrm{CF}_{}$ produced, two moles of $\mathrm{}_{2}$ are required.
$\text{Moles of } \mathrm{}_{2} =2 \times \text{Moles of } \mathrm{CF}_{}$

STEP 4

Plug in the given value for the moles of $\mathrm{CF}_{4}$ to calculate the moles of $\mathrm{}_{2}$ .
$\text{Moles of } \mathrm{}_{2} =2 \times3.25$

STEP 5

Calculate the moles of $\mathrm{}_{2}$ .
$\text{Moles of } \mathrm{}_{2} =2 \times3.25 =.5 \text{ moles}$

STEP 6

Now that we have the moles of $\mathrm{}_{2}$ , we can find the mass of $\mathrm{}_{2}$ required. We can do this by multiplying the moles of $\mathrm{}_{2}$ by the molar mass of $\mathrm{}_{2}$ .
$\text{Mass of } \mathrm{}_{2} = \text{Moles of } \mathrm{}_{2} \times \text{Molar mass of } \mathrm{}_{2}$

STEP 7

Plug in the values for the moles of $\mathrm{}_{2}$ and the molar mass of $\mathrm{}_{2}$ to calculate the mass of $\mathrm{}_{2}$ .
$\text{Mass of } \mathrm{}_{2} =6.5 \text{ moles} \times38.00 \mathrm{~g/mol}$

STEP 8

Calculate the mass of $\mathrm{}_{2}$ .
$\text{Mass of } \mathrm{}_{2} =6.5 \text{ moles} \times38.00 \mathrm{~g/mol} =247 \mathrm{~g}$ So,247 grams of fluorine, $\mathrm{}_{2}$ , are needed to generate3.25 moles of carbon tetrafluoride, $\mathrm{CF}_{4}$ .

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QuestionHow many grams of fluorine ( $\mathrm{F}_{2}$ ) are needed for 3.25 moles of carbon tetrafluoride ( $\mathrm{CF}_{4}$ )? Molar mass of $\mathrm{F}_{2}$ is 38.00 g/mol. [?] g $\mathrm{F}_{2}$

Studdy Solution

STEP 1

Assumptions1. The chemical reaction is balanced and proceeds to completion. . The molar mass of $\mathrm{}_{}$ is $38.00 \mathrm{~g/mol}$ .
3. We want to find the mass of $\mathrm{}_{}$ required to produce $3.25$ moles of $\mathrm{CF}_{4}$ .

STEP 2

First, we need to understand the stoichiometry of the reaction. From the balanced chemical equation, we can see that one mole of carbon reacts with two moles of fluorine to produce one mole of carbon tetrafluoride.
$\mathrm{C}+2 \mathrm{~}_{2} \rightarrow \mathrm{CF}_{4}$

STEP 3

STEP 4

Plug in the given value for the moles of $\mathrm{CF}_{4}$ to calculate the moles of $\mathrm{}_{2}$ .
$\text{Moles of } \mathrm{}_{2} =2 \times3.25$

STEP 5

Calculate the moles of $\mathrm{}_{2}$ .
$\text{Moles of } \mathrm{}_{2} =2 \times3.25 =.5 \text{ moles}$

STEP 6

STEP 7

Plug in the values for the moles of $\mathrm{}_{2}$ and the molar mass of $\mathrm{}_{2}$ to calculate the mass of $\mathrm{}_{2}$ .
$\text{Mass of } \mathrm{}_{2} =6.5 \text{ moles} \times38.00 \mathrm{~g/mol}$

STEP 8

Calculate the mass of $\mathrm{}_{2}$ .
$\text{Mass of } \mathrm{}_{2} =6.5 \text{ moles} \times38.00 \mathrm{~g/mol} =247 \mathrm{~g}$ So,247 grams of fluorine, $\mathrm{}_{2}$ , are needed to generate3.25 moles of carbon tetrafluoride, $\mathrm{CF}_{4}$ .

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QuestionHow many grams of fluorine (F2\mathrm{F}_{2}F2​) are needed for 3.25 moles of carbon tetrafluoride (CF4\mathrm{CF}_{4}CF4​)? Molar mass of F2\mathrm{F}_{2}F2​ is 38.00 g/mol. [?] g F2\mathrm{F}_{2}F2​

Studdy Solution

STEP 1

Assumptions1. The chemical reaction is balanced and proceeds to completion. . The molar mass of \mathrm{}_{}​ is 38.00 g/mol38.00 \mathrm{~g/mol}38.00 g/mol.3. We want to find the mass of \mathrm{}_{}​ required to produce 3.253.253.25 moles of CF4\mathrm{CF}_{4}CF4​.

STEP 2

First, we need to understand the stoichiometry of the reaction. From the balanced chemical equation, we can see that one mole of carbon reacts with two moles of fluorine to produce one mole of carbon tetrafluoride.C+2 2→CF4\mathrm{C}+2 \mathrm{~}_{2} \rightarrow \mathrm{CF}_{4}C+2 2​→CF4​

STEP 3

STEP 4

Plug in the given value for the moles of CF4\mathrm{CF}_{4}CF4​ to calculate the moles of 2\mathrm{}_{2}2​.Moles of 2=2×3.25\text{Moles of } \mathrm{}_{2} =2 \times3.25Moles of 2​=2×3.25

STEP 5

Calculate the moles of 2\mathrm{}_{2}2​.Moles of 2=2×3.25=.5 moles\text{Moles of } \mathrm{}_{2} =2 \times3.25 =.5 \text{ moles}Moles of 2​=2×3.25=.5 moles

STEP 6

STEP 7

Plug in the values for the moles of 2\mathrm{}_{2}2​ and the molar mass of 2\mathrm{}_{2}2​ to calculate the mass of 2\mathrm{}_{2}2​.Mass of 2=6.5 moles×38.00 g/mol\text{Mass of } \mathrm{}_{2} =6.5 \text{ moles} \times38.00 \mathrm{~g/mol}Mass of 2​=6.5 moles×38.00 g/mol

STEP 8

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QuestionHow many grams of fluorine ( $\mathrm{F}_{2}$ ) are needed for 3.25 moles of carbon tetrafluoride ( $\mathrm{CF}_{4}$ )? Molar mass of $\mathrm{F}_{2}$ is 38.00 g/mol. [?] g $\mathrm{F}_{2}$

Assumptions1. The chemical reaction is balanced and proceeds to completion. . The molar mass of $\mathrm{}_{}$ is $38.00 \mathrm{~g/mol}$ .
3. We want to find the mass of $\mathrm{}_{}$ required to produce $3.25$ moles of $\mathrm{CF}_{4}$ .

First, we need to understand the stoichiometry of the reaction. From the balanced chemical equation, we can see that one mole of carbon reacts with two moles of fluorine to produce one mole of carbon tetrafluoride.
$\mathrm{C}+2 \mathrm{~}_{2} \rightarrow \mathrm{CF}_{4}$

Plug in the given value for the moles of $\mathrm{CF}_{4}$ to calculate the moles of $\mathrm{}_{2}$ .
$\text{Moles of } \mathrm{}_{2} =2 \times3.25$

Calculate the moles of $\mathrm{}_{2}$ .
$\text{Moles of } \mathrm{}_{2} =2 \times3.25 =.5 \text{ moles}$

Plug in the values for the moles of $\mathrm{}_{2}$ and the molar mass of $\mathrm{}_{2}$ to calculate the mass of $\mathrm{}_{2}$ .
$\text{Mass of } \mathrm{}_{2} =6.5 \text{ moles} \times38.00 \mathrm{~g/mol}$