For the chemical reaction 2C4H10(g) + 13O2(g) â 8CO2(g) + 10H2O(â) assume that 10.6 g of C4H10 reacts completely to products. The density of CO2 is 1.96 g/L. What volume in liters of CO2 is produced?

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11 Dec 2019

For the chemical reaction 2C₄H₁₀(g) + 13O₂(g) â 8CO₂(g) + 10H₂O(â) assume that 10.6 g of C₄H₁₀ reacts completely to products. The density of CO₂ is 1.96 g/L. What volume in liters of CO₂ is produced?

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Butane undergoes combustion when it reacts with oxygen toproduce carbon dioxide and water. Using the ideal gas law equation,calculate the volume in liters, of oxygen needed to burn all thebutane at 0.850 atm and 25 degrees celsius if a tank contains 55.2g of butane.

2C4H10 (g) + 13O2 (g) ---> 8CO2 (g) + 10H2O (g)

Please show your work and have correct significant figures.Thank you!

The combustion of butane can be represented bythe following equation:

2C₄H₁₀ (g) + 13O₂(g)? 8CO₂(g) + 10H₂O(g)

If 256. g of C₄H₁₀ and 902. gO₂ react, which reactant is used up first? (enter butaneor oxygen) oxygen

Calculate the number of moles of the limiting reagent. Use thestoichiometry of the balanced equation to determine how many molesof CO₂ will be produced. Then convert this to grams ofCO₂ by using its molar mass.

1. What is the mass of carbondioxide produced? (Answer to 3 sig figs.) grams

2. What is the mass of water produced?(Answer to 3 sigfigs.) grams

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Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)â8CO2(g)+10H2O(l) At 1.00 atm and 23 âC, what is the volume of carbon dioxide formed by the combustion of 2.80 g of butane? what is the volume of CO2?The ideal gas law

PV=nRT

relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08206 Lâ atm/(Kâ mol)or 8.3145 J/(Kâ mol). The equation can be rearranged as follows to solve for n:

n=PVRT

This equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios.

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For the chemical reaction 2C₄H₁₀(g) + 13O₂(g) â 8CO₂(g) + 10H₂O(â) assume that 10.6 g of C₄H₁₀ reacts completely to products. The density of CO₂ is 1.96 g/L. What volume in liters of CO₂ is produced?

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For the chemical reaction 2C4H10(g) + 13O2(g) â 8CO2(g) + 10H2O(â) assume that 10.6 g of C4H10 reacts completely to products. The density of CO2 is 1.96 g/L. What volume in liters of CO2 is produced?

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Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

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For the chemical reaction 2C₄H₁₀(g) + 13O₂(g) â 8CO₂(g) + 10H₂O(â) assume that 10.6 g of C₄H₁₀ reacts completely to products. The density of CO₂ is 1.96 g/L. What volume in liters of CO₂ is produced?