HF is prepared by reacting CaF2 with H2 SO4: CaF2(s)+H2 SO4(ℓ) →2 HF(g)+CaSO4(s) HF can be elect

step 1 Number 130 is a little bit of Hess's Law and then some unit conversion and stoichiometry. So let

HF is prepared by reacting CaF2 with H2 SO4: CaF2(s)+H2...

HF is prepared by reacting $\mathrm{CaF}_{2}$ with $\mathrm{H}_{2} \mathrm{SO}_{4}:$ $$ \mathrm{CaF}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(\ell) \rightarrow 2 \mathrm{HF}(g)+\mathrm{CaSO}_{4}(s) $$ HF can be electrolyzed, in turn, when dissolved in molten KF to produce fluorine gas: $$ 2 \mathrm{HF}(\ell) \rightarrow \mathrm{F}_{2}(g)+\mathrm{H}_{2}(g) $$ Fluorine is extremely reactive, so it is typically sold as a $5 \%$ mixture by volume in an inert gas such as helium. How much $\mathrm{CaF}_{2}$ is required to produce $500.0 \mathrm{L}$ of $5 \% \mathrm{F}_{2}$ in helium? Assume the density of $\mathrm{F}_{2}$ gas is $1.70 \mathrm{g} / \mathrm{L}$

HF is prepared by reacting $\mathrm{CaF}_{2}$ with $\mathrm{H}_{2} \mathrm{SO}_{4}:$
$$
\mathrm{CaF}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(\ell) \rightarrow 2 \mathrm{HF}(g)+\mathrm{CaSO}_{4}(s)
$$
HF can be electrolyzed, in turn, when dissolved in molten KF to produce fluorine gas:
$$
2 \mathrm{HF}(\ell) \rightarrow \mathrm{F}_{2}(g)+\mathrm{H}_{2}(g)
$$
Fluorine is extremely reactive, so it is typically sold as a $5 \%$ mixture by volume in an inert gas such as helium. How much $\mathrm{CaF}_{2}$ is required to produce $500.0 \mathrm{L}$ of $5 \% \mathrm{F}_{2}$ in helium? Assume the density of $\mathrm{F}_{2}$ gas is $1.70 \mathrm{g} / \mathrm{L}$

Key Concepts

Mole Concept and Molar Mass

This concept is central to chemical calculations, as it connects the mass of a substance to the number of particles it contains via its molar mass. It allows the conversion between the mass of a compound and the amount in moles, serving as a bridge between macroscopic measurements and molecular-level stoichiometry.

Density and Mass Conversion for Gases

This concept involves using the density of a gas to convert between its volume and mass. By applying the relationship between mass, density, and volume, one can determine the total mass of a gas when its volume and density are known, which is essential for subsequent mole calculations.

Reaction Stoichiometry

This concept involves using the balanced chemical equations to relate the amounts of reactants and products in a chemical reaction. It requires understanding mole ratios and the step?by?step conversion from one substance to another through a series of reactions, allowing the calculation of how much of one reactant is needed to produce a certain amount of product.

Gas Mixture Composition

This concept concerns the understanding of mixtures of gases, particularly when a target gas is present as a defined percentage of the total volume. It involves calculating the actual volume or moles of the gas of interest from a given total volume of the gas mixture, using the percentage provided.

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