Complete combustion of 16 liters of gasoline consisting of a mixture of heptane gas (C7H16) and isooctane (C8H18) gas produces 124 liters of clean carbon dioxide gas in the air. a. what percentage each composition gas in gasoline? b. What volume of water vapor is released? c. If air contains 20% by volume of oxygen, what volume of air is required for this combustion?

Complete combustion of 16 liters of gasoline consisting of a mixture of heptane gas (C7H16) and isooctane (C8H18) gas produces 124 liters of clean carbon dioxide gas in the air. a. what percentage each composition gas in gasoline? b. What volume of water vapor is released? c. If air contains 20% by volume of oxygen, what volume of air is required for this combustion?

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter9: Energy For Today

Section: Chapter Questions

Problem 56E

See similar textbooks

Similar questions

You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1 volume gas X + 2 volumes gas Y 2 volumes compound I 2 volumes gas X + 1 volume gas Y 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
58 Magnesium will burn in air to form both Mg3N2 and MgO. What mass of each product would be found if burning a 3.11-g sample of magnesium to completion produces a combined total of 5.09 g of the two products?
A 230-L sample of a colorless gas at STP decomposed to give 230 L of N2 and 1.25 L of O2 at STP. What is the colorless gas?
62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1. volume gas X + 2 volumes gas Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
9.87 What will be the final temperature of a mixture made from equal masses of the following: water at 25.0 C, ethanol at 35.5 C, and iron at 95.0 C?
Propane, C3H8, is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for the complete combustion of propane gas. (b) Calculate the volume of air at 25 C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later chapter on gasesfor now use the information that 1.00 L of air at 25 C and 1.00 atm contains 0.275 g of 2 per liter.) (c) The heat of combustion of propane is 2,219.2 kJ/mol. Calculate the heat of formation, Hf of propane given that Hf of H2O(l)=285.8 kJ/mol and Hf of CO2(g)=393.5 kJ/mol. (d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.
An alternate way to state Avogadro’s law is A1l other things being equal, the number of molecules in a gas is directly proportional to the volume of the gas. (a) What is the meaning of the term directly proportional? (b) What are the other things that must be equal
Glycine is an amino acid made up of carbon, hydrogen, oxygen, and nitrogen atoms. Combustion of a 0.2036-g sample gives 132.9 mL of CO2 at 25C and 1.00 atm and 0.122 g of water. What are the percentages of carbon and hydrogen in glycine? Another sample of glycine weighing 0.2500 g is treated in such a way that all the nitrogen atoms are converted to N2(g). This gas has a volume of 40.8 mL at 25C and 1.00 atm. What is the percentage of nitrogen in glycine? What is the percentage of oxygen? What is the empirical formula of glycine?
A 36.0—L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO2, 805 g 02, and 4,880 g N2. At 25 degrees C. what is the pressure in the cylinder in atmospheres?