Chemistry, 04.04.2020 07:07 selfiegymnast

How many L of carbon dioxide at 1.00 atm and 298.15 K are released from a car's engine upon consumption of a 60.0 L LIQUID tank gasoline? (Gasoline density: 0.77 kg/L, Molar mass of C₈H₁₈: 114.2 g/mol) C₈H₁₈ (l) + ²⁵/₂ O₂ (g) → 8 CO₂ (g) + 9 H₂O (g)

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The liters L of carbon dioxide at 1.00 atm and 298.15 K released from the car's engine upon consumption of a 60.0 L LIQUID tank gasoline is 79230.76 L

From the given information;

The equation for the reaction can be expressed as:

$\mathbf{C_8H_8 _{(l)} + \frac{25}{2}O_2_{(g)} \to 8 CO_2_{(g)} + 9H_2O_{(g)}}$

Given that:

Pressure = 1.00 atmTemperature = 298.15 Kamount of gasoline used = 60.0 Lgasoline density = 0.77 kg/LMolar mass of C₈H₁₈: 114.2 g/mol

The first thing to do is to determine the mass amount of gasoline used by using the relation:

$\mathbf{Density = \dfrac{mass}{volume}}$

$\mathbf{0.77 \ kg/L = \dfrac{mass}{60 \ L}}}$

mass amount of gasoline used = 0.77 kg/L × 60 L

mass amount of gasoline used = 46.2 kg

mass amount of gasoline used = 46.2 × 1000g

mass amount of gasoline used = 46200 g

Now, since we know the mass amount of the gasoline used, we can determine the number of moles of the gasoline by using the formula:

$\mathbf{number of moles = \dfrac{mass}{molar \ mass}}$

$\mathbf{number of moles = \dfrac{46200 \ g}{114.2 \ g/mol}}$

$\mathbf{number \ of \ moles = 404.6 \ moles }$

From the given reaction, 1 mole of gasoline react to produce 8 moles of CO₂

As such, 404.6 moles of gasoline will produce = (404.6 moles × 8)/ 1

= 3236.8 moles of CO₂ is produced.

Now, using the ideal gas equation to determine the volume of CO₂ that are released;

PV = nRT

$\mathbf{1.00 atm \times V = 3236.8 moles \times 0.0821 atm L /K/mol \times 298.15 \ K}$

$\mathbf{V = \dfrac{3236.8 moles \times 0.0821 atm L /K/mol \times 298.15 \ K}{1.00 atm}}$

V = 79230.76 L

Therefore, we can conclude that the liters L of carbon dioxide at 1.00 atm and 298.15 K released from the car's engine upon consumption of a 60.0 L LIQUID tank gasoline is 79230.76 L

Learn more about ideal gas equation here:

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Answer from: ptrlvn01

79,000 liters

Explanation:

1. Number of moles of gasoline

a) Convert 60.0 liters to grams

density = 0.77kg/literdensity = mass / volumemass = density × volume mass = 0.77kg/liter × 60.0 liter = 46.2 kg46.2kg × 1,000g/kg = 46,200g

b) Convert 46,200 grams to moles

molar mass of C₈H₁₈ = 114.2 g/molnumber of moles = mass in grams / molar massnumber of moles = 46,200g / (114.2 gmol) = 404.55 mol

2. Number of moles of carbon dioxide, CO₂ produced

a) Balanced chemical equation (given):

C₈H₁₈ (l) + ²⁵/₂ O₂ (g) → 8 CO₂ (g) + 9 H₂O (g)

b) mole ratio:

1 mol C₈H₁₈ / 8 mol CO₂ = 404.55 mol C₈H₁₈ / x

Solve for x:

x = 404.55mol C₈H₁₈ × 8 mol CO₂ / 1mol C₈H₁₈ = 3,236.4 mol CO₂

3. Convert the number of moles of carbon dioxide to volume

Use the ideal gas equation:

pV = nRTV = nRT/pp = 1 atmT = 298.15Kn = 3,236.4 molR = 0.08206 (mol . liter)/ (K . mol)

Substitute and compute:

V =3,236.4 mol × 0.08206 (mol . liter) / (K . mol) 298.15K / 1 atmV = 79,183 liter

Round to two significant figures (because the density has two significant figures): 79,000 liters ← answer

Answer from: Quest

its mg hope this

Answer from: Quest

plants need sunlight, water, and carbon dioxide to make food. plants use the raw materials of water, nutrients they absorb from soil, and carbon dioxide to make sugars the plant can use. energy from the sun and chlorophyll are also needed.

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