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3 years ago

PLEASE HELP ME IM NOT SURE ABOUT THIS QUESTION

Chemistry

1 answer:

fgiga [73]3 years ago

8 0

Answer:

it is a

Explanation:

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Assuming that gasoline is 100% isooctane, that isooctane burns to produce only CO2CO2 and H2OH2O, and that the density of isooct

Aleksandr [31]

Answer:

1.12×10¹¹ kg of CO₂ are produced with 4.6×10¹⁰ L of isooctane

Explanation:

Let's state the combustion reaction:

C₈H₁₈ + 25/2O₂ → 8CO₂ + 9H₂O

Let's calculate the mass of isooctane that reacts.

Density = Mass / Volume

Density . Volume = Mass

First of all, let's convert the volume in L to mL, so we can use density.

4.6×10¹⁰ L . 1000 mL / 1L = 4.6×10¹³ mL

0.792 g/mL . 4.6×10¹³ mL = 3.64 ×10¹³ g

This mass of isooctane reacts to produce CO₂ and water, so let's determine the moles of reaction

3.64 ×10¹³ g . 1mol / 114 g = 3.19×10¹¹ mol

Ratio is 1:8 so 1 mol of isooctane can produce 8 moles of dioxide

Therefore 3.19×10¹¹ mol would produce (3.19×10¹¹ mol . 8) = 2.55×10¹² moles of CO₂

Now, we can determine the mass of produced CO₂ by multipling:

moles . molar mass

2.55×10¹² mol . 44 g/mol = 1.12×10¹⁴ g of CO₂

If we convert to kg 1.12×10¹⁴ g / 1000 = 1.12×10¹¹ kg

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3 years ago

A reaction was performed in which 4.0 g of cyclohexanol was reacted with an acid catalyst to obtain 2.8 g of cyclohexene. calcul

ioda

Answer:

%age Yield = 85.36 %

Solution:

The Balance Chemical Reaction is as follow,

C₆H₁₂O + Acid Catalyst → C₆H₁₀ + Acid Catalyst + H₂O

According to Equation ,

100 g (1 mole) C₆H₁₂O produces = 82 g (1 moles) of C₆H₁₀

So,

4.0 g of C₆H₁₂O will produce = X g of C₆H₁₀

Solving for X,

X = (4.0 g × 82 g) ÷ 100 g

X = 3.28 g of C₆H₁₀ (Theoretical Yield)

As we know,

%age Yield = (Actual Yield ÷ Theoretical Yield) × 100

%age Yield = (2.8 g ÷ 3.28 g) × 100

%age Yield = 85.36 %

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