2) The following series of reactions were carried out. PBCO3(s) + 2HNO3(aq) → Pb(NO3)2(aq) + H2O(1) + CO2(g) Pb(NO3)2(aq) + 2HC1(aq) → 2HNO3(aq) + PbCl2(s) of che (a) If a student starts with 2.871 g of lead(II) carbonate for the first reaction and all other reagents are added in excess, what is the theoretical yield of lead(II) chloride solid? Noie-ne oaposition oght about b ated. AB Sde replaceent ractins ly a metal) is added in solut ctive than the ion whilethe less active

2) The following series of reactions were carried out. PBCO3(s) + 2HNO3(aq) → Pb(NO3)2(aq) + H2O(1) + CO2(g) Pb(NO3)2(aq) + 2HC1(aq) → 2HNO3(aq) + PbCl2(s) of che (a) If a student starts with 2.871 g of lead(II) carbonate for the first reaction and all other reagents are added in excess, what is the theoretical yield of lead(II) chloride solid? Noie-ne oaposition oght about b ated. AB Sde replaceent ractins ly a metal) is added in solut ctive than the ion whilethe less active

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.13PAE: 3.13 An explosive whose chemical formula is C3H6N6O6 produces water, carbon dioxide, and nitrogen...

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3.83 For the reaction of nitrogen, N2, and hydrogen, H2, to form ammonia, NH3, a student is attempting to draw a particulate diagram, as shown below. Did the student draw a correct representation of the reaction? If not, what was the error the student made?
A sample of cocaine, C17H21O4N, is diluted with sugar, C12H22O11. When a 1.00-mg sample of this mixture is burned, 1.00 mL of carbon dioxide (d=1.80g/L) is formed. What is the percentage of cocaine in this mixture?
3.112 In one experiment, the burning of 0.614 g of sulfur produced 1.246 g of sulfur dioxide as its only product. In a second experiment run to verify the outcome of the first, a sample was burned and 0.813 g of sulfur dioxide was obtained, but the student running the experiment forgot to determine the initial mass of sulfur burned. Describe how the data already obtained could be used to calculate the initial mass of the sulfur burned in the second experiment.
You have a chemical in a sealed glass container filled with air. The setup is sitting on a balance as shown below. The chemical is ignited by means of a magnifying glass focusing sunlight on the reactant. After the chemical has completely burned, which of the following is true? Explain your answer. a. The balance will read less than 250.0 g. b. The balance will read 250.0 g. c. The balance will read greater than 250.0 g. d. The scales reading cannot be determined without knowing the identity of the chemical.
3.107 As computer processor speeds increase, it is necessary for engineers to increase the number of circuit elements packed into a given area. Individual circuit elements are often connected using very small copper “wires” deposited directly onto the surface of the chip. In some processors, these copper interconnects are about 22 nm wide. How many copper atoms would be in a 1-mm length of such an interconnect, assuming a square cross section? (The density of copper is 8.96 g/cm3.)
89 A number of compounds containing the heavier noble gases, and especially xenon, have been prepared. One of these is xenon hexafluoride (XeF6), which can be prepared by heating a mixture of xenon and fluoride gases. XeF6 is a white crystalline solid at room temperature and melts at about 325 K. A mixture of 0.0600 g of Xe and 0.0304 g of F2 is sealed into a 100.0-mL bulb. (The bulb is heated, and the reaction goes to completion. Then the sealed bulb is cooled back to 20.0°C. What will be the final pressure in the bulb, expressed in torr?
About 5 billion kilograms of benzene, C6H6, are made each year. Benzene is used as a starting material for many other compounds and as a solvent (although it is also a carcinogen, and its use is restricted). One compound that can be made from benzene is cyclohexane, C6H12. C6H6() + 3 H2(g) C6H12() rH = 206.7 kJ/mol-rxn; rS = 361.5 J/K mol-rxn Is this reaction predicted to be product-favored at equilibrium at 25 C? Is the reaction enthalpy- or entropy-driven?
3.13 An explosive whose chemical formula is C3H6N6O6 produces water, carbon dioxide, and nitrogen gas when detonated in oxygen. Write the chemical equation for the detonation reaction of this explosive.
According to NASA, the space shuttle's external fuel tank for the main propulsion system carries 7246 kg of liquid O2 and 283.2 kg of liquid H2. During takeoff, these chemicals react to form water as well as giving out a great amount of energy. ____ O2(g) + ____ H2(g) → ______ H2O How many kg of the excess reactant is left over?
When in danger, bombardier beetles can fire a hot, toxic mixture of chemicals at their attacker. This mixture contains quinone, C6H4O2, a compound that is formed by the reaction of hydroquinone, CH4(OH)2, with hydrogen peroxide, H2O2. The equation for the overall reaction is: CH4(OH)2(aq) + H2O2(aq) → C6H4O2(aq) + 2H2O(ℓ) Use the following data to calculate the enthalpy change, in kJ mol-1 , for the above reaction. CH4(OH)2(aq) → C6H4O2 (aq) + H2(g) ΔH = +177.4 kJ mol−1 H2(g) + O2(g) → H2O2(aq) ΔH = −191.2 kJ mol−1 H2(g) + ½O2(g) → H2O(g) ΔH = −241.8 kJ mol−1 H2O(g) → H2O(ℓ) ΔH = −43.8 kJ mol−1
Diiodine pentoxide is used in respirators to remove carbon monoxide from air. I2O5(s) + 5CO(g) → I2(s) + 5CO2(g)a) What mass of carbon monoxide could be removed from air by a respirator that contains 50.0 g of diiodine pentoxide, and what mass of I2 would remain in the respirator?
When Kay added 30g of Hydrochloric acid (HCI) to 65g of Zn, bubbles appeared and a white precipitate, zinc chloride (ZnCl2) was produced. She found that the mass of the zinc chloride was 93g. Since the law of conservation of matter stated that matter can’t be created or destroyed, she was puzzled about the difference in mass. What is the best explanation for the missing 2g?