(a)
Interpretation:Using the activity series inTable 15.3, indicate whether each of the following reactions is spontaneous:
Concept Introduction: The activity series of metals arranged from most active to least reactive:
Li > K> Ba> Ca> Na > Mg > Al > Zn > Cr > Fe > Cd > Ni > Sn > Pb > H> Cu > Ag >Hg > Pt> Au
Most active metals are easily oxidized and readily lose electrons as oxidation is the loss of electrons.
(b)
Interpretation: Using the activity series inTable 15.3, indicate whether each of the following reactions is spontaneous:
Concept Introduction:The activity series of metals arranged from most active to least reactive:
Li > K> Ba> Ca> Na > Mg > Al > Zn > Cr > Fe > Cd > Ni > Sn > Pb > H> Cu > Ag >Hg > Pt> Au
Most active metals are easily oxidized and readily lose electrons as oxidation is the loss of electrons.
(c)
Interpretation: Using the activity series inTable 15.3, indicate whether each of the following reactions is spontaneous:
Concept Introduction:The activity series of metals arranged from most active to least reactive:
Li > K> Ba> Ca> Na > Mg > Al > Zn > Cr > Fe > Cd > Ni > Sn > Pb > H> Cu > Ag >Hg > Pt> Au
Most active metals are easily oxidized and readily lose electrons as oxidation is the loss of electrons.
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Basic Chemistry
- nother reaction B is 73.10 (17.47 ). Assume a temperature of 298 K and 1M concentration. By what factor is one reaction faster than the other? Which reaction is faster? Reaction B is faster. O Reaction A is faster. Cannot be determined.arrow_forwardIs the following chemical reaction exothermic or endothermic? 31 (aq) + H3AS04(aq) + 2H* (aq) 13 (aq) + H3ASO3(aq) + H2O() AH°F(kJ/mole) S° (J/mole*K) Substance or ion -55.19 180.7 I (aq) -345.69 212.34 H3ASO4(aq) -11.23 11.09 H* (aq) 69.77 -89.6 13 (aq) H3ASO3(aq) -301.27 199.78 -285.8 69.95 H20 (1) endothermic then exothermic All I know is the reaction is cold to the toucharrow_forwardGiven the following data: 2H₂(g) + C(s) → CH4 (9) 2H₂(g) + O₂(g) → 2H₂O(1) C(s) + O₂(g) → CO₂ (9) Calculate AGⓇ for CH4 (9) +202 (g) → CO₂ (g) + 2H₂ O(1). AG: = kj A Go = -51 kJ A G° = -474 kJ A G = -394 kJarrow_forward
- (70 A K/s .l.a محمد Use Hess's law to Calculate AH (in kJ/mol) for the following reaction : CI, + F2(9) (g) CIF 3(9) Η ΔΗ, of H,0 μ. KJ/mol and AH°, of H,0 is -241.8 KJ/mol, then the ÄH°, of evaporation of H,ºL in ( KJ/mol) is : is -285.8 (g) Choose... Given the following thermochemical equation: 2C,H18() 16CO2 + 25 0,(g) 2(g) + 18 H,00 ΔΗ -11020 kJ/mol If AH°, [CO,lo = -393.5 kJ/mol 2(g) and AH°; [H,O = -285.8kJ/mol, calculate the standard enthalpy of formation of octane ( C,H,) in kJ/mol Choose...arrow_forward(23) Two aqueous solutions are both at room temperature and are then mixed in a coffee cup calorimeter. The reaction causes the temperature of the resulting solution to fall below room temperature. Which of the following statements is true? A) The products have a lower potential energy than the reactants. B) This type of experiment will provide data to calculate AErxn- C) The reaction is exothermic. D) Energy is leaving the system during reaction. E) None of the above statements are true.arrow_forwardQUESTION 16 For the the reaction coordinate shown here, write the appropriate labels for the given diagram saction coorde p of oction) AAGcat for example # 10 is free energy. Use the following labels. ES, AGxn , EXx AGr AGuncat"sAG Please put your answers in the answer box. What is the correct label for: a. 2 b. 3 с. 6 d. 8 e. 1 For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac) Arial 10pt Paragraph Cick Save and Subunit to save and submit Chick Sace All Ansuers t se all a e aE Moy coayarrow_forward
- In the "Méthode Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is C,H12Os (aq) + 2C, H;OH(aq) + 2002(9) Fermentation of 893 ml grape juice (density is 1.0 g/cm') is allowed to take place in a bottle with a total volume of 971 mL until 15% by volume is ethanol (C,H; OH). Assuming that CO2 obeys Henry's law, calculate the partial pressure of CO, in the gas phase and the solubility of CO, in the wine at 25°C. The Henry's law constant for CO, is 3.1 x 10-2 mol/L atm at 25°C with Henry's law in the form C = kP, where C is the concentration of the gas in mol/L. (The density of ethanol is 0.79 g/cm.) (Enter your answers to two significant figures.) Partial pressure atm Solubilityarrow_forwardIf you find that [CoCl42 (aq)] = 0.05 M, [Co(H₂O)62+ (aq)] = 0.43 M, and [CI-(aq)] = 0.707 M at 10 C, what is value of AG at 10 C, in kJ/mol? Express your response to two digits after the decimal. Question 5 A plot of AG (in units of kJ/mol) vs. T (K) yields a straight line with the equation: y = -14.67x + 268.8. What is the value of AH (kJ/mol) for the reaction, based on this data? Express your response to two digits after the decimal.arrow_forward22. Methanol, CH3OH (32.04 g/mol) has a melting point equal to 176 K and a boiling point equal to 338 K. Using the thermodynamic data below, calculate the amount of heat (kJ) required to convert 0.484 mol CH3OH from 115 K to 200 K. (15.51) (1) (mm) (3) 2.08 AHfusion = 2.2 kJ/mol AHvaporization = 35.2 kJ/mol A. 5.11 kJ Chloroform Acetone Temperature A. 162.9 torr B. 27.9 kJ Molar Mass (g/mol) Density (g/mL) 119.38 58.08 23. What is the total vapor pressure of a solution prepared by mixing 75.0 mL chloroform with 100.0 mL acetone. At the same temperature, their vapor pressures are 154.8 torr and 184.5 torr, respectively. A. 22.8 mL Csolid 105 J/mol-K Cliquid = 81.3 J/mol-K Cgas 48 J/mol-K B. 172.4 torr 1 C. 74.2 kJ 1.48 0.786 Vapor Pressure (torr) 154.8 184.5 C. 180.1 torr +484) (351) 176-115 = C. 43.3 mL 24. How many milliliters of ethanol (CH3CH₂OH, density = 0.791 g/mL, 32.04 g/mol) are required to prepare a 2.70 M solution with a total volume of 500.0 mL? 1 200 D. 131 kJ 10648 = 124…arrow_forward
- (Q77) The standard Gibbs free energy (AG°rxn) for the formation of sulfur trioxide from sulfur dioxide and oxygen gas is -72.3 kJ/mol. The balanced chemical equation is SO2 (g) + ½ O2 (g) --> SO3 (g). What will be the Gibbs Free energy of the reaction (in kJ/mol) if it takes place at a low temperature of -13.7 and the concentrations of three gases are: SO2 = 0.112 M %3D O2 = 0.110 M SO3 = 1.74 Marrow_forwardCalculate AH for the following reaction, given the data in the table below: 4N204 (2) →2N20g) + 4NO2 (g) + 302 AH = ??? kJ/mol 2NO2 (e) + 2NO() +O2 (g)→2N2O4 (g) AH = -396.81 kJ 4NO+ 2N2Og) + 502 (g)→4N2O4 (g) AH = -398.88 kJ 2NO + O2 ()→N2O4 (3) AH = -173.09 kJarrow_forwardGiven the following data 2 CIF(g) + O2 (g) Cl, 0(g)+F20(g) 2 CIF3 (9) +202 (g) Cl2 O(g) + 3F,0(g) 2F2 (9) + O2(9) 2F20(9) AH 167.4 kJ AH 341.4 kJ AH -43.4 kJ calculate AH for the reaction CIF(g) + F2(9) → CIF, (9) AH = k) Submit Answer Try Another Version 2 em attempts remaarrow_forward
- 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