An automobile gasoline tanks holds 18 kg of gasoline. When the gasoline burns, 72 kg of oxygen is consumed, and carbon dioxide and water are produced. What is the total combined mass in kg of carbon dioxide and water that is produced? Assume complete combustion. Enter your answer ONLY as a number; DO NOT include units.

Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and water. The unbalanced chemical equation for this reaction is given below: SO2(g)+NaOH(s)Na2SO3(s)+H2O(l) Assuming you react 38.3 g sulfur dioxide with 32.8 g sodium hydroxide and assuming that the reaction goes to completion, calculate the mass of each product formed.

Consider the following particulate-level representation of a chemical equation: The white spheres represent hydrogen atoms, the black sphere represents a carbon atom, and the red spheres represent oxygen atoms. a Write a balanced chemical equation representing this reaction. b Write a word description of the reaction on the particulate and molar levels.

When corn is allowed to ferment, the fructose in the corn is converted to ethyl alcohol according to the following reaction C6H12O6(aq)2C2H5OH(l)+2CO2(g)(a) What volume of ethyl alcohol (d=0.789g/mL) is produced from one pound of fructose? (b) Gasohol can be a mixture of 10 mL ethyl alcohol and 90 mL of gasoline. How many grams of fructose are required to produce the ethyl alcohol in one gallon of gasohol?

he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.

3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.

A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?

list at least three quantities that must be conserved in chemical reactions.

Magnesium ribbon reacts with acid to produce hydro- gen gas and magnesium ions. Different masses of magnesium ribbon are added to 10 mL of the acid. The volume of the hydrogen gas obtained is a measure of the number of moles of hydrogen produced by the reaction. Various measurements are given in the table below. (a) Draw a graph of the results by plotting the mass of Mg versus the volume of the hydrogen gas. (b) What is the limiting reactant in experiment 1? (c) What is the limiting reactant in experiment 3? (d) What is the limiting reactant in experiment 6? (e) Which experiment uses stoichiometric amounts of each reactant? (f) What volume of gas would be obtained if 0.300 g of Mg ribbon were used? If 0.010 g were used?

The reaction of an element X() with element Y() is represented in the following diagram. Which of the elements bestdescribes this reaction? mg src=Images/HTML_99425-6-16ALQ_image001.jpg alt="" align="top"/> msp;3X+6YX3Y8 msp;3X+6YX3Y6 msp;X+2YXY2 msp;3X+8Y3XY2+2Y