LWR # 1 Apply Stoichiometry A student performed an experiment to find the amount of sodium carbonate, (Na₂CO₂) that is produced from the decomposition of baking soda, NaHCO, by heating. Decomposition of baking soda: 2NaHCO,> Na₂CO, + CO₂ + H₂O The following data were collected. Complete the data table. Mass of empty evaporating dish 24.353 grams Mass of evaporating dish and baking 27.868 grams soda 26.885 grams Mass of evaporating dish and sodium carbonate Mass of baking soda 84.007 g/mol Mass of sodium carbonate (experimental) 105.9888 g/mol Molar mass of baking soda 84.007 g/mol Molar mass of sodium carbonate 105.9888 g/mol 1.678 grams > 4 Theoretical (calculated) mass of sodium carbonate 09314 g/mol Calculate percent error of the analysis (1105.9888-09314) +100/.09314 = 9.8% 1 = Atomic mass: Na = 23.0g; H=1.0 g; C=12.0g; O=16.0g % error = (Experimental-Calculated) x 100/ Calculated

LWR # 1 Apply Stoichiometry A student performed an experiment to find the amount of sodium carbonate, (Na₂CO₂) that is produced from the decomposition of baking soda, NaHCO, by heating. Decomposition of baking soda: 2NaHCO,> Na₂CO, + CO₂ + H₂O The following data were collected. Complete the data table. Mass of empty evaporating dish 24.353 grams Mass of evaporating dish and baking 27.868 grams soda 26.885 grams Mass of evaporating dish and sodium carbonate Mass of baking soda 84.007 g/mol Mass of sodium carbonate (experimental) 105.9888 g/mol Molar mass of baking soda 84.007 g/mol Molar mass of sodium carbonate 105.9888 g/mol 1.678 grams > 4 Theoretical (calculated) mass of sodium carbonate 09314 g/mol Calculate percent error of the analysis (1105.9888-09314) +100/.09314 = 9.8% 1 = Atomic mass: Na = 23.0g; H=1.0 g; C=12.0g; O=16.0g % error = (Experimental-Calculated) x 100/ Calculated

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 165MP

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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?
One of the components of polluted air is NO. It is formed in the high-temperature environment of internal combustion engines by the following reaction: N2(g)+O2(g)2NO(g)H=180KJ Why are high temperatures needed to convert N2 and O2 to NO?
Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)
Consider the accompanying diagram. Ball A is allowed to fall and strike ball B. Assume that all of ball As energy is transferred to ball B at point I, and that there is no loss of energy to other sources. What is the kinetic energy and the potential energy of ball B at point II? The potential energy is given by PE = mgz, where m is the mass in kilograms, g is the gravitational constant (9.81 m/s2), and z is the distance in meters.
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
How does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?
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?
The introduction to this chapter says that "we live immersed in a gaseous solution.” What dues. that mean?
A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.
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.
Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.
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?

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