Question
In: Chemistry
Consider the following balanced equation for the combustion of butane, a fuel often used in lighters:...
Consider the following balanced equation for the combustion of butane, a fuel often used in lighters:
2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g)
Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed.
| Mass C4H10C4H10 | Mass O2O2 | Mass CO2CO2 | Mass H2OH2O |
| _____ | 2.11 gg | _____ | _____ |
| 5.52 gg | _____ | _____ | _____ |
| _____ | _____ | 10.12 gg | _____ |
| _____ | _____ | _____ | 8.04 gg |
| 222 mgmg | _____ | _____ | _____ |
| _____ | _____ | 128 mgmg | _____ |
Solutions
Expert Solution
Here we are asked to find mass of reactants and products
We use conversion factors from balanced reaction
2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g)
Mass of C4H10 =
=0.588 g C4H10
Similarly we can solve for products
Mass of CO2 =
Mass of H2O =
-------------------------------------------------------------------------------------------------
In the next row we are given with Mass of C4H10 = 5.52 g
Mass of O2 required =
Mass of CO2 formed =
Mass of H2O formed =
Similarly we can solve remaining blanks
queen_honey_blossom answered 1 year agoRelated Solutions
Consider the following balanced equation for the combustion of butane, a fuel often used in lighters....
Consider the following balanced equation for the combustion of
butane, a fuel often used in lighters.
2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g) Complete the following table,
showing the appropriate masses of reactants and products. If the
mass of a reactant is provided, fill in the mass of other reactants
required to completely react with the given mass, as well as the
mass of each product formed. If the mass of a product is provided,
fill in the required masses of each reactant to make that...
Consider the following balanced equation for the combustion of butane, a fuel often used in lighters:...
Consider the following balanced equation for the combustion of
butane, a fuel often used in lighters:
2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g)
Complete the following table, showing the appropriate masses of
reactants and products. If the mass of a reactant is provided, fill
in the mass of other reactants required to completely react with
the given mass, as well as the mass of each product formed. If the
mass of a product is provided, fill in the required masses of each
reactant to make that...
The balanced equation for the combustion of butane is: 2C4H10 +13O2-->8CO2 + 10H2) If the combustion...
The balanced equation for the combustion of butane is: 2C4H10
+13O2-->8CO2 + 10H2)
If the combustion of 42.0 g of C4H10
produces 103 g of CO2. What is the percent yield of the
reaction? (Assume oxygen is in excess.)
Write the balanced reaction equation for the complete combustion of butane, C4H10, in air. Determine the...
Write the balanced reaction equation for the complete combustion
of butane, C4H10, in air. Determine the mass
and mole fractions of fuel, oxygen and nitrogen in the reactants.
Also, determine the mass and mole fraction of carbon dioxide in the
products. Determine the mass and mole air-fuel ratios.
Write a balanced equation for the combustion of gaseous methane? Another potential future fuel is methanol...
Write a balanced equation for the combustion of gaseous methane?
Another potential future fuel is methanol (CH3OH). Write a balanced equation for the combustion of gaseous methanol?
Express your answer as a chemical formula.
Another potential future fuel is methanol (CH3OH). Use bond energies to calculate the enthalpy of combustion of methanol in kJ/mol.
Express your answer in kiloJoules to three significant figures.
Use bond energies to calculate AH rxn for this reaction: N2(g) + 3H2(g) rightarrow 2NH3(g)....
1. Write a balanced equation for the complete combustion of each of the following: a. 2,2-dimethylbutane...
1. Write a balanced equation for the complete combustion of each
of the following:
a. 2,2-dimethylbutane
Express your answer as a chemical equation. Identify all of the
phases in your answer.
b. cyclopentane
Express your answer as a chemical equation. Identify all of the
phases in your answer.
2. Consider the compound ethylcyclopentane
a. Write the equation for the complete combustion of
ethylcyclopentane.
Express your answer as a chemical equation.
b. Calculate the grams O2 required for the reaction of...
For each of the following, write a balanced chemical equation. Combustion of glycerol, CH2OHCHOHCH2OH, yields carbon...
For each of the following, write a balanced chemical
equation.
Combustion of glycerol, CH2OHCHOHCH2OH, yields carbon dioxide
and water.
Solid silver phosphate and an aqueous solution of potassium
nitrate formed when aqueous solutions of silver nitrate and
potassium phosphate were combined.
Cu2+(aq) + I−(aq) → CuI(s) +
I3−(aq)
Lead (II) nitrate solution is added to potassium iodide
solution, solid lead (II) iodide forms and potassium nitrate
solution remains.
Liquid disilicon hexachloride reacts with water to form solid
silicon dioxide, hydrogen...
Hydrogen fuel has been used in fuel cells or internal combustion engines. Determine the heat of...
Hydrogen fuel has been used in fuel cells or internal combustion
engines. Determine the heat of combustion, energy capacity, and
carbon footprint of the fuel.
ΔHf H2O(l) = -285.8 kJ/mol
A. . The balanced equation for the combustion of ethanol is 2C2H5OH(g) + 7O2(g) 4CO2(g)...
A. . The balanced equation for the combustion of ethanol is
2C2H5OH(g) + 7O2(g) 4CO2(g) + 6H2O(g) How many grams of dioxygen
are required to burn 5.9 g of C2H5OH? B. 2Al(s) + 6HCl(aq)
2AlCl3(aq) + 3H2(g) According to the equation above, how many grams
of aluminum are needed to completely react with 3.83 mol of
hydrochloric acid? C. What is the formula for the chlorate of
gadolinium(III)? D. What is the formula for the nitride of
samarium(III)?...
A combustion process consumes 1.25 g/s of fuel. The fuel has a heat of combustion of...
A combustion process consumes 1.25 g/s of fuel. The fuel has a
heat of combustion of 45 MJ/kg.
The air flow rate is 19 g/s and the air enters the engine at 300 K,
1 atm. Determine:
(1) The outlet temperature of the air.
(2) The air-fuel ratio
(3) The heat added to the air.
* Assume the cold-air standard model applies.
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- JAVASCRIPT: Please create an array of student names and another array of student grades. - Create...
- Topic - Construction: Structural, loads, tension 1.) Explain why pure tension members are the most efficient...
- Procter and Gamble (PG) paid an annual dividend of $ 1.62$1.62 in 2009. You expect PG...
- locate a recent case of online child pornography. Write a summary of the incident and describe...
- #Python 5. Write function called evaluate() that evaluates the following Python expressions or assignments as specified:...
- Suggest journal, research paper link reference. i need this as reference for writing a research with...
- Cryptography is used heavily in internet communications. True or false? Explain
ADVERTISEMENT