The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18)(C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 4.2 kgkg of octane burned. ( HintHint: Begin by writing a balanced equation for the combustion reaction.)

Butane, C4H10C4H10, 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)→8CO2(g)+10H2O(l)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atmatm and 23 ∘C∘C, what is the volume of carbon dioxide formed by the combustion of 1.60 gg of butane?

Gasoline is primarily composed of iso-octane, which has the chemical formula C8H18. When gasoline is burned, the chemical equation is: 2C8H18  +  25O2  --->  16CO2 + 18H2O This means that 2 molecules of iso-octane combine with 25 oxygen molecules to produce 16 carbon dioxide molecules and 18 water molecules. Use of fossil fuels adds CO2, carbon dioxide, to the atmosphere. This human-generated CO2 increases the planetary greenhouse effect, leading to an increase in average land surface temperatures, accumulation of heat in the oceans, and modification of global climate. Part of the problem is that a lot of CO2 is produced per mass of fuel burned. You can see that by looking at the fraction of carbon in iso-octane and carbon dioxide. 1. Calculate the formula masses of iso-octane (C8H18) and carbon dioxide (CO2) 2. What is the percent composition of carbon (C) in C8H18 and CO2?

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1. A sample of 2.8 g of Al(s) reacts with a sample of 4.15 g of Cla(g) according to the following chemical equation: Alu+ClaAlCl How many grams of AICI, will be produced if the reaction is carried out at 70% efficiency?

Consider the following reaction: CO(g)+2H2(g)=CH3OH(g). Determine the theoretical yield of methanol (CH3OH) in grams.

Do not give handwriting solution.

Catalytic converters are the most common option for controlling emissions of polluting gases by internal combustion engines in automobiles, accelerating the conversion of nitrogen oxides into nitrogen and oxygen gases. A chemical reaction that can be used for the conversion of nitric oxide into non-polluting gases is the reaction of this gas with hydrogen, resulting in nitrogen and water gases, as shown in the chemical equation below: 2 NO(g) + 2 H2(g) → N2(g) + H2O(g) The kinetics of this reaction at a temperature of 1250 °C is represented in the following table, which indicates the influence of the concentration of the reactants on the reaction rate, obtained through three experiments conducted under the same conditions EXPERIMENTO [NO] (MOL/L) [H2] (MOL/L) V0 (MOL/Ls) 1 0,20 0,08 0,05 2 0,40 0,08 0,20 3 0,40 0,16 0,40 Determine the rate law for this chemical reaction, the rate constant, and its respective unit. Calculate the rate when the concentration of NO is 0.30…

The balanced equation for the combustion of butane, CAH10, is shown below. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 CAH10(g) + 13 02(g) --> 8 CO2(g) + 10 H20(1) 58.124 32 44.011 18.016 How many liters of oxygen gas would be necessary to burn 18.2 g of butane?

Bromobenzene (C6H5Br) is obtained with the reaction between benzene (C6H6) and bromine gas (Br2). Write the balanced equation. Use the equal sign as a substitute to the arrow sign. Follow this format: 2H2 + O2 = 2H2O