CHEM 1301 Chapter Notes - Chapter 3: Photosynthesis, Bond Energy, University Of Manchester

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blushseal731

22 Nov 2017

School

University of Manitoba

Department

Chemistry

Course

CHEM 1301

Professor

Sarrah Vakili

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Document Summary

Chemistry 1300- chapter 3 notes (pg 130-136 and 114-119) Recognizing the types of energy interest to chemists. Types of energy: matter: anything that occupies space and possesses mass, energy: the capacity to do work, work: the displacement of an object against an opposing force. It"s the e(cid:374)ergy fro(cid:373) positi(cid:448)e a(cid:374)d (cid:374)egati(cid:448)e io(cid:374)s held a s(cid:373)all dista(cid:374)(cid:272)e apart: energy electrical= kq1q2 r. Where q1 and q2 are the charges of two ions, r is the distance between the ions, and k= 2. 31 x 10^-16 j pm. Chemical energy is energy resulting from attraction of the electrons and nuclei in molecules (bond energy) Bond formation releases energy: thermal: form of energy associated with the motion of small particles of matter. Mass of a body is a measure of its energy content. Mass transformation of mass into energy (e=mc^2), where c is the speed of light.

Related Questions

An instrument used to measure the pressure of a gas in a laboratory is called a barometer manometer sphygmomanometer spectrophotometer spectrometer The pressure of a gas in a container is1.85 atm and occupies a volume of 12.5 L If the original volume is reduced by hall at constant temperature, what would happen to the pressure? The pressure would ... double reduce by half remain the same On a hot summer day, you notice that a bag of chips left in your vehicle has inflated. As temperature increased, gas molecules .......... kinetic energy and the volume of gas inside the bag ....... Lost/increased gained/decreased lost/decreased gained/increased What mass of oxygen gas (O_2) is needed to fill a 585 L tank at STP? 0 835 kg 0.765 kg 0.417 kg Which of the following will cause the volume of an ideal gas to triple in value Raising the temperature from 25 degree C to 75 degree C at constant pressure. Lowering the absolute temperature by a factor of 3 at constant pressure. Lowering the pressure by a factor of 3 white the temperature stays constant. A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm. What is the identity of the halogen? Br_2 F_2 C1_2 l_2 Define vapor pressure. partial pressure cf water in a Squid mixture partial pressure of wafer in a gases mixture condensation of water A mixture of 1.0 mol He and 1.0 mol No are at STP in a rigid container. Which of the following statements is TRUE Both gases have the same average kinetic energy. Both gases contribute equally to the density of the mixture under these conditions. Both gases have the same molecular speed. The following reaction is used to generate hydrogen gas in the laboratory Mg(s) + 2 HC1(aq) rightarrow MgC1_2(aq) + H_2(g) If 243 mL of gas is collected at 25 degree C and has a total pressure of 745 mm Hg. what mass of hydrogen is produced? Listed are vapor pressures at select temperatures: Listed are water vapor Pressures at select temperatures: 0.0144 g H_2 0.0717 g H_2 0.0190 g H_2 Which of the following compounds will behave LEAST like an ideal gas at low temperatures? He SO_2 H_2 N_2 F_2 A container Filed with neon and argon gas is 25.00% by volume neon. What is the partial pressure of argon it the total pressure inside the container is 5 500 atm? 412 5 atm 1.375 atm 4.125atm 28 5 L of an unknown gas has a mass of 55.92 g at STP. What is the identity of the unknown gas? CO_2 O_2 N_2 Explain what would happen to the following equilibrium upon the addition of more hydrogen gas? H_2O(g) + CO(g) doubleheadarrow H_2(g) + CO_2(g) producing more reactants producing more CO_2 equilibrium will not be attected For the following reaction, K_5 = 5.6 x 10^-6 (at 400 K): 2 NOC(g) doubleheadarrow 2 No_2(g) + C1_2(g) If [NOCI] = 0.0222 M, [CI_2] = 0.0222 M, [NO_2] = 0.989 M at once, which statement would be true? The rate of forward and reverse reaction are equal. Neither forward nor reverse reaction would occur. Rate of forward reaction would be taster. Rate of reverse reaction would be faster. K_c = 1.10 times 10^18 for CO(g) + 1/2 O_2(g) doubleheadarrow CO_2(g) Calculate the equilibrium concstant K_0 for the following CO_2(g) doubleheadarrow CO(g) + 1/2 O_2(g) 1.04 times 10^9 0.55 times 10^18 -1.10 times 10^18 9.09 times 10^19

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 1301 Chapter Notes - Chapter 3: Photosynthesis, Bond Energy, University Of Manchester

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