Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
(1) A metal that gets covered with a protective film of its oxide (Al, Cu, Ag)
(2) A metal which burns in air with golden flame (Zn, K, Na)
(3) A metal which can displace hydrogen from boiling water as well as steam (K, Zn, Fe)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 2 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 1)State the First Law of Thermodynamics. 2)Fluorine (F2) and iodine (I2) are both Group 17 elements. Explain with reference to intermolecular forces, why fluorine is a gas and iodine is a solid at room temperature. 4)When 30 g of ammonium nitrate, (NH4NO3) was stirred into 10 cm3 of water, the temperature fell from 21 oC to 15 oC. 5)Calculate the total amount of energy (E) released in this experiment. Ignore the heat capacity of ammonium nitrate. Take the specific heat capacity of the water as 4.18 J g-1 ºC-1. Density of water is 1.00 gcm-3. 6)This amount of energy [answer to part (i)] was produced by 30 g of ammonium nitrate. Calculate the energy change per mole of ammonium nitrate. Include the correct sign for…arrow_forward2 (a) In this investigation, you will use a polystyrene-cup calorimter to determine the amount of heat released during acid-base neutralization reactions. Find information in your textbook, an encyclopedia, or a web site about calorimetry. Sketch the apparatus for a polystrene-cup calorimeter. (b) For more precise heat of reaction measurnments, chemists use a device called bomb calorimeter. How is a bomb calorimeter similar to and different from a polystyrene-cup calorimeter?arrow_forwardO Discuss the factors affecting the sign of AG in the relationship AG= AH - TAS. Give examples for each of the situations,arrow_forward
- The Ostwald process for the commercial production of nitric acid involves three steps. 4 NH3(g) + 5 02(9) 4 NO(g) + 6 H20(g) 2 NO(g) + 02(g) → 2 NO2(g) 3 NO2(g) + H20(1) → 2 HNO3(/) + NO(g) (a) Calculate AH°, AS°, AG°, and K (at 298 K) for each of the three steps in the Ostwald process (see Appendix 4). (Use the values you calculate for AH° and AS° to calculate AG°.) first step second step third step AH° -908 V kJ ΔΗ -112 V kJ AH° -74 kJ AS° 181 V J/K AS° -147 V J/K AS° |-267 V J/K AG° -928 V kJ AG° -70 V kJ AG° 6 x kJ K 0.11 K 1.03 K 0.089 (b) Calculate the equilibrium constant for the first step at 825°C, assuming AH° and AS° do not depend on temperature. 41.45 (c) Is there a thermodynamic reason for the high temperature in the first step assuming standard conditions? O Yes O No Explain. > > > xarrow_forwardAcetylene gas, C2H21g2, is used in welding. What is the maximum amount of useful work that can be accomplished under standard conditions by this reaction?arrow_forwardAlkali metals are often used to remove traces of water from organic solvents, such as diethyl ether. Because the reaction (see below) releases heat, care must be taken to make sure that the solvent does not "boil over". 2 Na(s) + 2 H₂O(1) ➜ 2 NaOH(aq) + H₂(g) a) Determine the standard enthalpy change for this reaction. Comment on the relative strength of bonding and/or interactions in the products vs reactants, and briefly explain how you decided this. Substance Na(s) H₂O(1) NaOH(aq) H₂(g) AHºf (kJ/mol) 0 -285.83 -469.15 0 b) How much heat (in kJ) is released via the reaction of 1.00 g of sodium metal with water? If this much heat is released into 275 g of diethyl ether initially at 25°C, will the solvent reach its boiling point? If so, how many grams of the ether will evaporate? Show calculations to support your answer. For diethyl ether: Cs = 2.51 J/g⋅K, b.p. = 35°C, heat of vaporization = 377 J/g.arrow_forward
- (a) Draw a Lewis diagram for carbonic acid, H,CO3, with a central carbon atóm bonded to the three oxygen atoms. (b) Carbonic acid is unstable in aqueous solution and converts to dissolved carbon dioxide. Use bond enthal- pies to estimate the enthalpy change for the following reaction: H,CO;→ H,O + CO,arrow_forwardThe hydrocarbons acetylene (C2H2) and benzene (C6H6)have the same empirical formula. Benzene is an “aromatic”hydrocarbon, one that is unusually stable because of its structure.(a) By using data in Appendix C, determine the standardenthalpy change for the reaction 3 C2H2(g)-----> C6H6(l).(b) Which has greater enthalpy, 3 mol of acetylene gas or1 mol of liquid benzene? (c) Determine the fuel value, inkJ/g, for acetylene and benzene.arrow_forward(28) The standard Gibbs free energy associated with the following reaction is -91.2 kJ: HCI (g) + NH3 (g) → NH,CI (s) What will be the value of AG,nn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atm and the partial pressure of NH3 (g) is 0.284 atm? (A) (B) -95.1 kl -90.7 kl (C) (D) (E) 3.93 kJ noltemol or ni lu bluos noinsou -79.5 kJ -87.3 kJarrow_forward
- Using the data in the plot below, calculate the value of the enthalpy of the reaction (in kJ/mol) for this reaction: Fe (ag) + SCN (aq) 4 FESCN** (aq) 2+ y = 1986.9x-1.5206 R? = 0.9979 5.7 5.6 InKc 5.5 5.4 5.3 5.2 5.1 4.9 0.00325 0.0033 0.00335 0.0034 0.00345 0.0035 0.00355 0.0036 0.00365 1/Tarrow_forwardCan you help me out with this one please. Thank you.arrow_forward(b) What is the first law of thermodynamic? Define the Hess law. Given the following data; 2CIF(g) + 0,(g) CI,0(g) + F,O(g) AH = 167.4 kJ AH = 341.4 kJ SH = -43,4 kJ 2CIF,(g) + 20,(g) → CĻ0(g) + 3F,O(g) 2F,(2) + O(8) → 2F,O(g) calculate AH for the reaction CIF(g) + F(8) CIF,(g)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY