CHEM 1122 Lecture Notes - Lecture 9: Joule, Lead, Alkaline Earth Metal

26 views4 pages

chocolatealligator971

29 Oct 2018

School

Department

Course

Professor

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

Heat a(cid:296)d e(cid:296)ergy (cid:656) joule (cid:706)j(cid:707) = (cid:656) k(cid:258) (cid:295)^(cid:657) s^-(cid:657) (cid:656) calo(cid:336)ie (cid:706)the e(cid:296)e(cid:336)(cid:258)(cid:383) (cid:296)eeded to (cid:336)aise the te(cid:295)pe(cid:336)atu(cid:336)e o(cid:257) (cid:656) (cid:258) o(cid:257) (cid:377)ate(cid:336) (cid:656) de(cid:258)(cid:336)ee c (cid:656) cal = (cid:659). (cid:656)(cid:663)(cid:659) j. Nut(cid:336)itio(cid:296)al calo(cid:336)ie o(cid:336) calo(cid:336)ie (cid:706) c (cid:707) o(cid:257) kcal = (cid:656)(cid:655)(cid:655)(cid:655) calo(cid:336)ies. E(cid:296)e(cid:336)(cid:258)(cid:383) (cid:706)cal o(cid:336) cal(cid:707) = (cid:295)ass (cid:382) cha(cid:296)(cid:258)e i(cid:296) 9. B(cid:383) e(cid:295)itti(cid:296)(cid:258) pa(cid:336)ticles, (cid:336)adioacti(cid:376)e ele(cid:295)e(cid:296)ts/ato(cid:295)s ca(cid:296) beco(cid:295)e a di(cid:257)(cid:257)e(cid:336)e(cid:296)t ele(cid:295)e(cid:296)t. W(cid:336)ite the (cid:296)uclea(cid:336) e(cid:335)uatio(cid:296)s (cid:257)o(cid:336) the (cid:257)ollo(cid:377)i(cid:296)(cid:258) (cid:659)(cid:655)/(cid:656)(cid:664) k -> (cid:659)(cid:655)/(cid:656)(cid:663) a(cid:336) + (cid:655)/+(cid:656) e. (cid:657)(cid:657)(cid:663)/(cid:663)(cid:663) ra -> (cid:657)(cid:657)(cid:659)/(cid:663)(cid:661) r(cid:296) + (cid:659)/(cid:657) he. Ga(cid:295)(cid:295)a e(cid:295)issio(cid:296) o(cid:257) iodi(cid:296)e-(cid:656)(cid:658)(cid:656) (cid:706)(cid:655)/(cid:655) (cid:258)a(cid:295)(cid:295)a(cid:707) (cid:656)(cid:658)(cid:656)/(cid:660)(cid:658) i -> (cid:656)(cid:658)(cid:656)/(cid:660)(cid:658) i + (cid:655)/(cid:655) (cid:258)a(cid:295)(cid:295)a. G(cid:336)oup (cid:656)a = alkali (cid:295)etals (cid:706)+(cid:656)(cid:707) na + , li + , k + etc . G(cid:336)oup (cid:657)a = alkali(cid:296)e ea(cid:336)th (cid:295)etals (cid:706)+(cid:657)(cid:707) ca (cid:657)+ , m(cid:258) (cid:657)+ , etc . A(cid:258) = a(cid:258) + , cu(cid:706)ii(cid:707) = cu (cid:657)+ , cu(cid:706)i(cid:707) = cu + , fe(cid:706)iii(cid:707) = fe (cid:658)+

Related Questions

Question 2 Energy Calculations

a) Calculate the heat energy (q) when 12.0 g of water is heated from 20oC to 100oC. The

specific heat for water is given in your textbook.

b) Is the process of heating water exothermic or endothermic? Explain your answer.

Question 3 Energy Calculations

You dissolve 0.1 mol of ammonium nitrate in 100 mL of H2O. The temperature of the solution

changes from 22oC to 15oC. The specific heat capacity for water is 4.184 J/g.K. Show all

calculations on a separate sheet of paper!

a) Is this reaction endothermic or exothermic?

b) Calculate the heat, q, released or absorbed in the dissolution reaction.

c) Calculate the enthalpy change, ?Hrxn (kJ/mol), for dissolving 1 mol of ammonium nitrate.

Question 4. A gas expands from 264 mL to 971 mL at constant temperature. Calculate

the amount of work done in Joules by the gas when it expands against a constant pressure of 955

torr.

Question 5 Energy Calculations

a) The nutritional calorie (Calorie) is equivalent to 1 kcal. One pound (1.0 lb) of body fat is

equivalent to 4.1 x 103 kcal. Express this quantity in joules and kilojoules. Use

scientific notation for your answer!

b) If an athlete expends 1850 kJ/h (kilojoules per hour), how long does he have to exercise

to work off 1.0 lb of body fat?

c) The average amount of calories burned during running is 125 kcal/mile. How many

miles does this athlete have to run to burn off 1.0 lb of body fat?

Question 6

Calculate ?Ho for the following reactions at 298 K. Give the balanced thermochemical

equations and show the correct physical state in each equation. Calculate the enthalpy change

for each reaction. You will find thermochemical data in the back of your textbook in Appendix 3

(p. A-8 to A-12)

a) The formation of 1 mol of HCl (gas) from its elements

b) The formation of 1 mol of sodium chloride from its elements

c) The combustion of 1 mol glucose to water and carbon dioxide

d) HCl(g) + NH3(g) ? NH4Cl(g)

Question 7

Calculate heat of formation of SO2 under nonstandard state conditions, given the following

equations

SO2(g) +

Could you please answer these questions

++++++

++++++++

+++++++

++++++

+++++++

++++++

+++++++

++++++++

thank you

For a particular reaction, DeltaH = -111.4 kJ and DeltaS = -25.0 J/K. Calculate DeltaG for this reaction at 298 K Classify the following phase changes by the signs of the system's DeltaH and DeltaS. Consider these reactions, where M represents a generic metal. Use the information above to determine the enthalpy of the following reaction. Consider these reactions, where M represents a generic metal. 2M(s) + 6HCl(aq) rightarrow 2MCl3(aq) + 3H2(s) Delta H1, = -650.0 kJ HCl(g) rightarrow HCI(aq) Delta H2 = -74.8 kJ H2(g)+Cl2(g) rightarrow 2HC1(g) Delta H3 = -1845.0kJ MCI3(S) rightarrow MCI3(aq) Delta H4 = -416.0kJ Use the information above to determine the enthalpy of the following reaction 2M(S) + 3CI2(g) rightarrow 2MCI3(S) Delta H = A researcher studying the nutritional value of a new candy places a 4.20-gram sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.17 degree C. If the heat capacity of the calorimeter is 34.00 kJ K-1, how many nutritional Calories are there per gram of the candy? When 1.250 x 103 J of heat energy is added to 43.5 g of hexane, C6H14, the temperature increases by 12.7 degree C. Calculate the molar heat capacity of C6H14. If you have 420.0 mL of water at 25.00 degree C and add 130.0 mL of water at 95.00 degree C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water. A 54.21 g sample of a substance is initially at 24.2 degree C. After absorbing 2755 J of heat, the temperature of the substance is 108.6 degreeC. What is the specific heat (c) of the substance? If a system has 325 kcal of work done to it, and releases 5.00 times 102 kJ of heat into its surroundings, what is the change in internal energy of the system? Classify each of the following as a path function or a state function. A 1687 kg car is traveling down the road at 105.0 km/h. While traveling at this rate of speed, what is the kinetic energy of this vehicle in kilojoules? Convert the following energy units, 451 kJ to J 2060 kcal to kJ 9.77 x 106 J to kcal

Practice problems for exam 2 ______________

Useful Information:

h=6.626Ã10-34JÂ·s.; c=3.0Ã108 m/sec; E=hï® ; E= hc , ï¬ = h/mv; 1J = 1 kg-m2/s2 ï¬

mass of electron = 9.11 Ã 10-28 g, ïE= q + w ; 1 cal = 4.184 Joules Please Show all Work

1. Which of the following substances have standard heats of formation that are equal to zero by definition (circle your answers): H2(g), H(g), O3(g), H2O(s), H2O(l), Hg(l), Hg(s), Hg(g).

2. Limestone stalactites are formed in the reaction: Ca2+(aq) + HCO3-(aq) ï CaCO3(s) + CO2(g) +

H2O(l)
If one mole of CaCO3 is produced at 298 K under one atmosphere of pressure, the reaction performs 590 calories of expansion work, pushing back the atmosphere as CO2 is formed. At the same time, 9310 calories of heat are absorbed from the environment. What is ïE in Kcal/mole for CaCO3.

3. What is the minimum wavelength of light in AÌ (1 AÌ = 10-8 cm) needed to provide enough energy per quantum to rupture the chemical bond in hydrogen iodide (HI). The bond dissociation energy of HI is 71.4 Kcal/mole.

4. Sketch the shape and orientation of the following types of orbitals: s, px, dxy, dz2, dx2-y2

5. Give the values of (n) , (l) and (ml) for each orbital in the 4p subshell.

6. Write the complete electron configuration for the following: Ti 2+_____________________________________ Cr_______________________________________

N______________________________________

7. Calculate the standard enthalpy of formation ( ï Ho) for diamond from graphite [i.e. C (graphite) ï C (diamond)] given that:

C (graphite) + O2 ï CO2 (g) ( ï Ho = -393.5 KJ/mole) C (diamond)] + O2 ï CO2 (g) ( ï Ho = -395.4 KJ/mole)

If 1.0g of graphite is converted to diamond, what is the energy change? Is this an endothermic or exothermic reaction?

8. An 160 pound astronaut on his way to Mars is buzzing along at 10,000 miles per hour. (a) Express his weight in grams (one pound = 454 grams) so that you can calculate the astronautâs wavelength (1mile/hour = 44.7 cm/sec)

(b) Suppose the astronaut detects outside his spacecraft a proton (m=1.7 x 10-24 g) from a âsolar windâ moving at exactly the spacecraft velocity. What is the proton wavelength is in AÌ (1 AÌ = 10-8 cm.

9. What is the maximum number of electrons that can occupy each of the following subshells? a) 3d_________________ b) 1s____________________ c) 2p ____________________

10. Identify the element represented by the following electronic configuration.

a) [Ne] 3s2____________________

b) What is the electron configuration for the first excited state of this atom.______________

11. Determine the number of valence electrons for each element.
(a) Br___________ (b) Na _________ (c) Sn __________

12. 175 g of Fe at 15.0oC is mixed with 225 g of H2O at 95.0oC. What is the final temperature of the mixture? The specific heats of iron= 0.448 J/g oC and water = 4.184 J/g oC). (keep in mind the following: heat gained + heat lost = 0 and q=mass x heat capacity x ïT)

13. (5 pts) Calculate values of ÎHrxn for the following reactions: CS2(g) + 3O2(g) ï® CO2(g) + 2SO2(g)

The heat of formation for the following substances is given in kJ/mol:

CS2 CO2 SO2 117.4 -393.51 -296.83

14. (6 pts) Use the electron configuration of Li and Be and determine which element has the greatest second ionization energy. Defend your answer.

15. Mark beside each of the following processes either âexoâ or âendoâ according to whether you think the process will release heat or absorb heat.

a. Ca(g) ï Ca(g)+2 + 2e-
b. I(g)+1e-ï I(g)-1
c. Ca(g)+2 + S(g)-2 ï CaS(s) d. I2(g)ï 2I(g)

( ) ( ) ( ) ( )

16. (6 pts) In each of the following pairs, which of the two species is larger?
a) O-2 or Na+ b) Ti+4 or Ti+2 c) B or C d) N or N-3

17. Write down the Lewis dot structure for the following (a) N_______________ (b) Ne________________

18. THE BORN HABER CYCLE: I may have a problem on the Born Haber cycle. Please check my lecture notes to see how to set up the process and then calculate the lattice energy from the various thermodynamic quantities such as in the NaCl example below;

ï H ï¯ f NaCl = -411KJ

Na(s) ï® Na(g) ï H =108KJ
1â2 Cl2 ï® Cl(g) ï H = 122KJ Ionization Energy of Na ï H = 496 KJ Electron affinity of Cl ï H = -349KJ

CHEM 1122 Lecture Notes - Lecture 9: Joule, Lead, Alkaline Earth Metal

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 1122 Lecture Notes - Lecture 6: Orange Oil, Vinaigrette, Heat Capacity

CHMA10H3 Chapter Notes - Chapter 6: Coffee Cup, Enthalpy, Exothermic Process

CHM 103 Lecture Notes - Lecture 12: State Function, Kinetic Energy, Calorie

Related Questions