CHEMISTRY-ALEKS 360 ACCESS
13th Edition
ISBN: 9781260994742
Author: Chang
Publisher: MCG
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Chapter 18.6, Problem 1RCF
How many Leclanché cells are contained in a 9-volt battery?
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When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.
When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.
Which experimental number must be initialled by the Lab TA for the first run of Part 1 of the experiment?
a) the heat capacity of the calorimeter
b) Mass of sample
c) Ti
d) The molarity of the HCl
e) Tf
Predict products for the Following organic rxn/s by
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Chapter 18 Solutions
CHEMISTRY-ALEKS 360 ACCESS
Ch. 18.1 - Balance the following equation for the reaction in...Ch. 18.1 - Determine the number of electrons transferred in...Ch. 18.1 - For the following reaction in acidic solution,...Ch. 18.2 - Write the cell diagram for the following redox...Ch. 18.2 - Write the balanced redox reaction corresponding to...Ch. 18.3 - Can Sn reduce Zn2+(aq) under standard-state...Ch. 18.3 - What is the standard emf of a galvanic cell made...Ch. 18.3 - Prob. 1RCFCh. 18.3 - Prob. 2RCFCh. 18.4 - Prob. 4PE
Ch. 18.4 - Prob. 5PECh. 18.4 - Calculate the equilibrium constant for the...Ch. 18.4 - Prob. 2RCFCh. 18.4 - Prob. 3RCFCh. 18.5 - Prob. 6PECh. 18.5 - Prob. 7PECh. 18.5 - Consider the following cell diagram:...Ch. 18.5 - Calculate the cell voltage at 25C of a...Ch. 18.6 - How many Leclanch cells are contained in a 9-volt...Ch. 18.7 - Prob. 1RCFCh. 18.8 - An aqueous solution of Mg(NO3)2 is electrolyzed....Ch. 18.8 - A constant current is passed through an...Ch. 18.8 - What is the minimum voltage needed for the...Ch. 18.8 - Prob. 2RCFCh. 18.8 - In the electrolysis of molten CaCl2, a current of...Ch. 18 - Balance the following redox equations by the...Ch. 18 - Balance the following redox equations by the...Ch. 18 - Define the following terms: anode, cathode, cell...Ch. 18 - Describe the basic features of a galvanic cell....Ch. 18 - What is the function of a salt bridge? What kind...Ch. 18 - What is a cell diagram? Write the cell diagram for...Ch. 18 - What is the difference between the half-reactions...Ch. 18 - Prob. 18.8QPCh. 18 - Use the information in Table 2.1, and calculate...Ch. 18 - Discuss the spontaneity of an electrochemical...Ch. 18 - Calculate the standard emf of a cell that uses the...Ch. 18 - Calculate the standard emf of a cell that uses...Ch. 18 - Predict whether Fe3+ can oxidize I to I2 under...Ch. 18 - Which of the following reagents can oxidize H2O to...Ch. 18 - Consider the following half-reactions:...Ch. 18 - Predict whether the following reactions would...Ch. 18 - Which species in each pair is a better oxidizing...Ch. 18 - Which species in each pair is a better reducing...Ch. 18 - Consider the electrochemical reaction Sn2+ + X Sn...Ch. 18 - The Ecell for the following cell is 1.54 V at 25C:...Ch. 18 - Write the equations relating G and K to the...Ch. 18 - Prob. 18.22QPCh. 18 - Prob. 18.23QPCh. 18 - The equilibrium constant for the reaction...Ch. 18 - Use the standard reduction potentials to find the...Ch. 18 - Calculate G and Kc for the following reactions at...Ch. 18 - Under standard-state conditions, what spontaneous...Ch. 18 - Given that E = 0.52 V for the reduction...Ch. 18 - Prob. 18.29QPCh. 18 - Write the Nernst equation for the following...Ch. 18 - What is the potential of a cell made up of Zn/Zn2+...Ch. 18 - Calculate E, E, and G for the following cell...Ch. 18 - Calculate the standard potential of the cell...Ch. 18 - Referring to the arrangement in Figure 18.1,...Ch. 18 - Calculate the emf of the following concentration...Ch. 18 - Explain the differences between a primary galvanic...Ch. 18 - Discuss the advantages and disadvantages of fuel...Ch. 18 - The hydrogen-oxygen fuel cell is described in...Ch. 18 - Calculate the standard emf of the propane fuel...Ch. 18 - Prob. 18.41QPCh. 18 - Galvanized iron is steel sheet that has been...Ch. 18 - Tarnished silver contains Ag2S. The tarnish can be...Ch. 18 - Prob. 18.44QPCh. 18 - What is the difference between a galvanic cell...Ch. 18 - Describe the electrolysis of an aqueous solution...Ch. 18 - The half-reaction at an electrode is...Ch. 18 - Consider the electrolysis of molten barium...Ch. 18 - Prob. 18.49QPCh. 18 - If the cost of electricity to produce magnesium by...Ch. 18 - One of the half-reactions for the electrolysis of...Ch. 18 - How many moles of electrons are required to...Ch. 18 - Calculate the amounts of Cu and Br2 produced in...Ch. 18 - In the electrolysis of an aqueous AgNO3 solution,...Ch. 18 - A steady current was passed through molten CoSO4...Ch. 18 - A constant electric current flows for 3.75 h...Ch. 18 - What is the hourly production rate of chlorine gas...Ch. 18 - Chromium plating is applied by electrolysis to...Ch. 18 - The passage of a current of 0.750 A for 25.0 min...Ch. 18 - A quantity of 0.300 g of copper was deposited from...Ch. 18 - In a certain electrolysis experiment, 1.44 g of Ag...Ch. 18 - One of the half-reactions for the electrolysis of...Ch. 18 - A steady current of 10.0 A is passed through three...Ch. 18 - Industrially, copper metal can be purified...Ch. 18 - A Daniell cell consists of a zinc electrode in...Ch. 18 - A concentration cell is constructed having Cu...Ch. 18 - For each of the following redox reactions, (i)...Ch. 18 - The oxidation of 25.0 mL of a solution containing...Ch. 18 - The SO2 present in air is mainly responsible for...Ch. 18 - Prob. 18.70QPCh. 18 - Prob. 18.71QPCh. 18 - Oxalic acid (H2C2O4) is present in many plants and...Ch. 18 - Prob. 18.73QPCh. 18 - Prob. 18.74QPCh. 18 - From the following information, calculate the...Ch. 18 - Consider a galvanic cell composed of the SHE and a...Ch. 18 - A galvanic cell consists of a silver electrode in...Ch. 18 - Prob. 18.78QPCh. 18 - Calculate the emf of the following concentration...Ch. 18 - Prob. 18.80QPCh. 18 - Suppose you are asked to verify experimentally the...Ch. 18 - Prob. 18.82QPCh. 18 - An aqueous KI solution to which a few drops of...Ch. 18 - A piece of magnesium metal weighing 1.56 g is...Ch. 18 - Prob. 18.85QPCh. 18 - An acidified solution was electrolyzed using...Ch. 18 - In a certain electrolysis experiment involving...Ch. 18 - Consider the oxidation of ammonia:...Ch. 18 - When an aqueous solution containing gold(III) salt...Ch. 18 - In an electrolysis experiment, a student passes...Ch. 18 - People living in cold-climate countries where...Ch. 18 - Given that...Ch. 18 - A galvanic cell with Ecell = 0.30 V can be...Ch. 18 - Shown here is a galvanic cell connected to an...Ch. 18 - Fluorine (F2) is obtained by the electrolysis of...Ch. 18 - A 300-mL solution of NaCl was electrolyzed for...Ch. 18 - Industrially, copper is purified by electrolysis....Ch. 18 - An aqueous solution of a platinum salt is...Ch. 18 - Consider a galvanic cell consisting of a magnesium...Ch. 18 - A current of 6.00 A passes through an electrolytic...Ch. 18 - Prob. 18.101QPCh. 18 - Explain why most useful galvanic cells give...Ch. 18 - The table here shows the standard reduction...Ch. 18 - Consider a concentration cell made of the...Ch. 18 - A silver rod and a SHE are dipped into a saturated...Ch. 18 - Zinc is an amphoteric metal; that is, it reacts...Ch. 18 - Use the data in Table 18.1 to determine whether or...Ch. 18 - The magnitudes (but not the signs) of the standard...Ch. 18 - A galvanic cell is constructed as follows. One...Ch. 18 - Given the standard reduction potential for Au3+ in...Ch. 18 - Prob. 18.111QPCh. 18 - When 25.0 mL of a solution containing both Fe2+...Ch. 18 - Consider the Daniell cell in Figure 18.1. When...Ch. 18 - Use the data in Table 18.1 to show that the...Ch. 18 - Consider two electrolytic cells A and B. Cell A...Ch. 18 - A galvanic cell consists of a Mg electrode in a 1...Ch. 18 - The concentration of sulfuric acid in the...Ch. 18 - Consider a Daniell cell operating under...Ch. 18 - An electrolysis cell was constructed similar to...Ch. 18 - Prob. 18.120QPCh. 18 - Prob. 18.121QPCh. 18 - Prob. 18.122QPCh. 18 - A piece of magnesium ribbon and a copper wire are...Ch. 18 - The zinc-air battery shows much promise for...Ch. 18 - Calculate E for the reactions of mercury with (a)...Ch. 18 - Because all alkali metals react with water, it is...Ch. 18 - A galvanic cell using Mg/Mg2+ and Cu/Cu2+...Ch. 18 - Given the following standard reduction potentials,...Ch. 18 - Compare the pros and cons of a fuel cell, such as...Ch. 18 - Lead storage batteries are rated by ampere hours,...Ch. 18 - Use Equations (17.10) and (18.3) to calculate the...Ch. 18 - A construction company is installing an iron...Ch. 18 - A 9.00 102-mL 0.200 M MgI2 was electrolyzed. As a...Ch. 18 - Based on the following standard reduction...Ch. 18 - Calculate the equilibrium constant for the...Ch. 18 - The nitrite ion (NO2) in soil is oxidized to...Ch. 18 - The diagram here shows an electrolytic cell...Ch. 18 - Fluorine is a highly reactive gas that attacks...Ch. 18 - Show a sketch of a galvanic concentration cell....Ch. 18 - The emf of galvanic cells varies with temperature...Ch. 18 - A concentration cell ceases to operate when the...Ch. 18 - It has been suggested that a car can be powered...Ch. 18 - Estimate how long it would take to electroplate a...Ch. 18 - The potential for a cell based on the standard...
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- When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.arrow_forwardQ6: Using acetic acid as the acid, write the balanced chemical equation for the protonation of the two bases shown (on the -NH2). Include curved arrows to show the mechanism. O₂N- O₂N. -NH2 -NH2 a) Which of the two Bronsted bases above is the stronger base? Why? b) Identify the conjugate acids and conjugate bases for the reactants. c) Identify the Lewis acids and bases in the reactions.arrow_forwardQ5: For the two reactions below: a) Use curved electron-pushing arrows to show the mechanism for the reaction in the forward direction. Redraw the compounds to explicitly illustrate all bonds that are broken and all bonds that are formed. b) Label Bronsted acids and bases in the left side of the reactions. c) For reaction A, which anionic species is the weakest base? Which neutral compound is the stronger acid? Is the forward or reverse reaction favored? d) Label Lewis acids and bases, nucleophiles and electrophiles in the left side of the reactions. A. 용 CH3OH я хон CH3O OH B. HBr CH3ONa NaBr CH3OHarrow_forward
- potential energy Br b) Translate the Newman projection below to its wedge-and-dash drawing. F H. OH CH3 CI c) Isopentane (2-methylbutane) is a compound containing a branched carbon chain. Draw a Newman projection of six conformations about the C2-C3 bond of isopentane. On the curve of potential energy versus angle of internal rotation for isopentane, label each energy maximum and minimum with one of the conformations. 0° 。 F A B D C angle of internal rotation E F 360° (=0°) JDownlarrow_forwardQ7: Identify the functional groups in these molecules a) CH 3 b) Aspirin: HO 'N' Capsaicin HO O CH3 CH 3arrow_forwardQ2: Name the following alkanesarrow_forward
- 1. Complete the following table in your laboratory notebook. Substance Formula Methanol CH3OH Ethanol C2H5OH 1-Propanol C3H7OH 1-Butanol C4H9OH Pentane C5H12 Hexane C6H14 Water H₂O Acetone C3H60 Structural Formula Molecular Weight (g/mol) Hydrogen Bond (Yes or No)arrow_forwardQ1: Compare the relative acidity in each pair of compounds. Briefly explain. (a) CH3OH vs NH 3 (b) HF vs CH3COOH (c) NH3 vs CH4 (d) HCI vs HI (e) CH3COOH vs CH3SH (f) H₂C=CH2 vs CH3 CH3 (g) compare the acidity of the two bolded hydrogens O. H N- (h) compare the acidity of the two bolded hydrogens, draw resonance structures to explain H H Harrow_forwardQ3: Rank the following molecules in order of decreasing boiling point: (a) 3-methylheptane; (b) octane; (c) 2,4-dimethylhexane; (d) 2,2,4-trimethylpentane.arrow_forward
- Q5: Conformations of Alkanes a) Draw a Newman Projection of the compound below about the C2-C3 bond. H3C Cli... H IIIH Br CH3arrow_forwardThe ability of atoms to associate with each other depends ona) the electronic structure and its spatial orientation.b) the electron affinity.c) The other two answers are correct.arrow_forwardWhat is the final volume after you reach the final temperature? I put 1.73 but the answer is wrong not sure why The initial volume of gas is 1.60 LL , the initial temperature of the gas is 23.0 °C°C , and the system is in equilibrium with an external pressure of 1.2 bar (given by the sum of a 1 bar atmospheric pressure and a 0.2 bar pressure due to a brick that rests on top of the piston). Then, as you did in Exercise 1, you heat the gas slowly until the temperature reaches 48.2 °Carrow_forward
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