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Fittoniya [83]
3 years ago
6

You have arrived on a planet where S2, not O2, is the gas used as fuel in combustion reactions. When gaseous propane (C3H8) is b

urned in S2, H2S and carbon disulfide gases are produced. If 200.0 grams of propane and 75.0 grams of S2 were reacted, what is the theoretical yield of carbon disulfide. Include balance equations
Chemistry
1 answer:
Debora [2.8K]3 years ago
8 0

Answer:

Mass = 53.45 g

Explanation:

Given data:

Mass of propane = 200 g

Mass of S₂ = 75 g

Theoretical yield /Mass of CS₂ = ?

Solution:

Balanced Chemical equation:

C₃H₈ + 5S₂      →    4H₂S + 3CS₂

Number of moles of propane:

Number of moles = mass / molar mass

Number of moles = 200 g/  44.1 g/mol

Number of moles = 4.54 mol

Number of moles of S₂:

Number of moles = mass / molar mass

Number of moles = 75 g/  64.14 g/mol

Number of moles = 1.17 mol

Now we will compare the moles of carbon disulfide with both reactant.

                        S₂             :           CS₂

                         5              :            3

                        1.17           :          3/5×1.17 = 0.702

                       C₃H₈          :            CS₂

                           1             :               3

                        4.54          :              3×4.54 = 13.62 mol

Number of moles of CS₂ produced by S₂ are less so it will limiting reactant and limit the yield of carbon disulfide.

Theoretical yield of carbon disulfide.

Mass = number of moles ×molar mass

Mass = 0.702 mol × 76.14 g/mol

Mass = 53.45 g

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To prepare 350 mL of 0.100 M solution from a 1.50 M solution, we simply have to use the formula:

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1.50 M * V1 = 0.100 M * 350 mL

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Considering the Hess's Law, the enthalpy change for the reaction is 221.8 kJ/mol.

Hess's Law indicates that the enthalpy change in a chemical reaction will be the same whether it occurs in a single stage or in several stages. That is, the sum of the ∆H of each stage of the reaction will give us a value equal to the ∆H of the reaction when it occurs in a single stage.

In this case you want to calculate the enthalpy change of:

C₂H₄ (g) + 6 F₂ (g) → 2 CF₄ (g) + 4 HF (g)

which occurs in three stages.

You know the following reactions, with their corresponding enthalpies:

Equation 1: H₂ (g) + F₂ (g) → 2 HF (g)     ∆H° = -79.2 kJ/mol

Equation 2: C (s) + 2 F₂ (g) → CF₄ (g)     ∆H° = 141.3 kJ/mol

Equation 3: 2 C(s) + 2 H₂ (g) → C₂H₄ (g)     ∆H° = -97.6 kJ/mol

Because of the way formation reactions are defined, any chemical reaction can be written as a combination of formation reactions, some going forward and some going back.

<h3 /><h3>FIRST STEP</h3>

First, to obtain the enthalpy of the desired chemical reaction you need one mole of C₂H₄ (g) on reactant side and it is present in first equation. Since this equation has one mole of C₂H₄ (g) on the product side, it is necessary to locate it on the reactant side (invert it).

When an equation is inverted, the sign of ΔH° also changes.

<h3>SECOND STEP</h3>

Now, you need 2 moles of CF₄ (g) on the product side. The second equation has 1 mole of CF₄ (g) on the product side, so it is necessary to multiply it by 2 to obtain 2 moles of CF₄ (g).

Since enthalpy is an extensive property, that is, it depends on the amount of matter present, since the equation is multiply by 2, the variation of enthalpy also.

<h3>THIRD STEP</h3>

Finally, you need 4 moles of  HF (g) on the product side. The first equation has 2 moles of  HF (g) on the product side, so it is necessary to multiply it by 2 to obtain 4 moles of the compound.

Since the equation is multiply by 2, the variation of enthalpy also is multiplied by 2.

<h3>SUMMARY</h3>

In summary, you know that three equations with their corresponding enthalpies are:

Equation 1: 2 H₂ (g) + 2 F₂ (g) → 4 HF (g)     ∆H° = -158.4 kJ/mol

Equation 2: 2 C (s) + 4 F₂ (g) → 2 CF₄ (g)     ∆H° = 282.6 kJ/mol

Equation 3: C₂H₄ (g) → 2 C(s) + 2 H₂ (g)     ∆H° = 97.6 kJ/mol

Adding or canceling the reactants and products as appropriate, and adding the enthalpies algebraically, you obtain:

C₂H₄ (g) + 6 F₂ (g) → 2 CF₄ (g) + 4 HF (g)     ΔH°= 221.8 kJ/mol

Finally, the enthalpy change for the reaction is 221.8 kJ/mol.

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