1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Sidana [21]
2 years ago
15

Assuming gasoline is 89.0% isooctane, with a density of 0.692 g/mL, what is the theoretical yield (in grams) of CO2 produced by

the combustion of 1.80 x 1010 gallons of gasoline (the estimated annual consumption of gasoline in the U.S.)? Remember, there are 3.785 liters in 1 gallon and assume that isooctane is the only carbon containing component of gasoline. Scientific notation can be entered as follows: 1.23 x 1023 = 1.23E23
Chemistry
1 answer:
AfilCa [17]2 years ago
6 0

<u>Answer:</u> The theoretical yield of carbon dioxide is 1.453\times 10^{14}g

<u>Explanation:</u>

We are given:

Volume of isooctane = 1.80\times 10^{10}gallons

To convert this into liters, we use the conversion factor:

1 gallon = 3.785 L

So, 1.80\times 10^{10}gallon\times (\frac{3.785L}{1gallon})=6.813\times 10^{10}L

To calculate the mass of isooctane, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

Volume of isooctane = 6.813\times 10^{10}L=6.813\times 10^{13}mL    (Conversion factor:  1 L = 1000 mL)

Density of isooctane = 0.692 g/mL

Putting values in above equation, we get:

0.692g/mL=\frac{\text{Mass of isooctane}}{6.813\times 10^{13}mL}\\\\\text{Mass of isooctane}=(0.692g/mL\times 6.813\times 10^{13}mL)=4.714\times 10^{13}g

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

Given mass of isooctane = 4.714\times 10^{13}g

Molar mass of isooctane = 114.22 g/mol

Putting values in equation 1, we get:

\text{Moles of isooctane}=\frac{4.714\times 10^{13}g}{114.22g/mol}=4.127\times 10^{11}mol

The chemical equation for the combustion of isooctane follows:

2C_8H_{18}+25O_2\rightarrow 16CO_2+18H_2O

By Stoichiometry of the reaction;

2 moles of isooctane produces 16 moles of carbon dioxide.

So, 4.127\times 10^{11}mol of isooctane will produce = \frac{16}{2}\times 4.127\times 10^{11}mol=3.3016\times 10^{12}mol of carbon dioxide

  • Now, calculating the mass of carbon dioxide from equation 1, we get:

Molar mass of carbon dioxide = 44.00 g/mol

Moles of carbon dioxide = 3.3016\times 10^{12}mol

Putting values in equation 1, we get:

3.3016\times 10^{12}mol=\frac{\text{Mass of carbon dioxide}}{44.00g/mol}\\\\\text{Mass of carbon dioxide}=(3.3016\times 10^{12}mol\times 44.00g/mol)=1.453\times 10^{14}g

Hence, the theoretical yield of carbon dioxide is 1.453\times 10^{14}g

You might be interested in
Which option contains a correct statement about the size of
Vinil7 [7]

Answer:

a molecule always has two or more atoms

5 0
1 year ago
For the reaction KClO2⟶KCl+O2 KClO2⟶KCl+O2 assign oxidation numbers to each element on each side of the equation. K in KClO2:K i
frosja888 [35]

Answer:

Explanation:

The formula of the reaction:

            KClO₂ → KCl + O₂

To assign oxidation numbers, we have to obey some rules:

  1. Elements in an uncombined state or one whose atoms combine with one another to form molecules have an oxidation number of zero.
  2. The charge on simple ions signifies their oxidation number.
  3. The algebraic sum of all the oxidation number of all atoms in a neutral compound is zero. For radicals with charges, their oxidation number is the charge.

The oxidation number of K in KClO₂:

                                   K + (-1) + 2(-2) = 0

                                    K-5 = 0

                                    K = +5

The oxidation number of K in KCl:

                                K + (-1) = 0

                                K = +1

The oxidation number Cl in KClO₂ is -1

For Cl in KCl, the oxidation number is -1

For O in KClO₂, the oxidation number is (2 x -2) = -4

For O in O₂, the oxidation number is 0

K moves from an oxidation state of +5 to +1. This is a gain of electrons and K has undergone reduction. We then say K is reduced.

O moves from an oxidation state of -4 to 0. This is a loss of electrons and O has undergone oxidation. We say O is oxidized.

7 0
3 years ago
Read 2 more answers
If I initially have a gas at a pressure of 12 kPa, a volume of 23 liters, and a temperature of 200 K, and then I raise the press
sertanlavr [38]

Answer:

The new volume of gas would be 30 L.

Explanation:

This is an example of a Combined Gas Laws problem.

5 0
3 years ago
How will vinegar slow down the break down of an apple?
Gennadij [26K]

Answer:

Many people take apple cider vinegar before protein-heavy meals to improve digestion. The theory is that apple cider vinegar increases the acidity of your stomach, which helps your body create more pepsin, the enzyme that breaks down protein

5 0
2 years ago
a 125 g chunk of aluminum at 182 degrees Celsius was added to a bucket filled with 365 g of water at 22.0 degrees Celsius. Ignor
Diano4ka-milaya [45]
<h3>Answer:</h3>

32.98°C

<h3>Explanation:</h3>

We are given the following;

Mass of Aluminium as 125 g

Initial temperature of Aluminium as 182°C

Mass of water as 265 g

Initial temperature of water as 22°C

We are required to calculate the final temperature of the two compounds;

First, we need to know the specific heat capacity of each;

Specific heat capacity of Aluminium is 0.9 J/g°C

Specific heat capacity of water is 4.184 J/g°C

<h3>Step 1: Calculate the Quantity of heat gained by water.</h3>

Assuming the final temperature is X°C

we know, Q = mcΔT

Change in temperature, ΔT = (X-22)°C

therefore;

Q = 365 g × 4.184 J/g°C × (X-22)°C

    = (1527.16X-33,597.52) Joules

<h3>Step 2: Calculate the quantity of heat released by Aluminium </h3>

Using the final temperature, X°C

Change in temperature, ΔT = -(X°- 182°)C (negative because heat was lost)

Therefore;

Q = 125 g × 0.90 J/g°C × (182°-X°)C

  = (20,475- 112.5X) Joules

<h3>Step 3: Calculating the final temperature</h3>

We need to know that the heat released by aluminium is equal to heat absorbed by water.

Therefore;

(20,475- 112.5X) Joules = (1527.16X-33,597.52) Joules

Combining the like terms;

1639.66X = 54072.52

             X = 32.978°C

                = 32.98°C

Therefore, the final temperature of the two compounds will be 32.98°C

7 0
3 years ago
Other questions:
  • This process of heat transfer by conduction would NOT work __________
    5·2 answers
  • 2.5 moles of oxygen react with 3.5 moles of hydrogen according to the following balance equation: 2H2 + 1 O2 —&gt; 2 H2O. What i
    9·1 answer
  • A substance whose water solution is a good conductor of electricity is an ________
    11·1 answer
  • Explain the relationship between the volume of a gas and it’s pressure.
    14·1 answer
  • How are the boiling point and freezing point of a solvent affected when a solute is added?
    15·2 answers
  • Calculate the rate speed per drop in minute when applying a drip of 1000mg to last 4 2 hours​
    7·1 answer
  • Fill in the blanks for
    11·2 answers
  • 6. Is the following equation balanced or
    8·1 answer
  • A face centered cubic cell has an edge length of 495 pm. What is that atomic radius?
    14·1 answer
  • Name the following alkane:
    7·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!