A. Beta emission is associated with: (SELECT ALL THAT APPLY)

a, b, c, d, e, f, g

B. Electron-capture is associated with: (ALL THAT APPLY)

a, b, c, d, e, f, g

C. Alpha emission is associated with (ALL THAT APPLY)

a, b, c, d, e, f, g

D. Positron emission is associated with (SELECT ALL THAT APPLY)

a, b, c, d, e, f, g

a. increase in mass number

b. emission of a photon

c. decrease in mass number

d. conversion of a proton to a neutron

e. decrease in atomic number

f. increase in atomic number

g. conversion of a neutron to a proton

For Kl and lithium phosphate give the cation name and symbol, anion name and symbol, and chemical formula.

Which is an impossible ectron configuration?

1s22s2

1s32s22p4

1s22s22p4

1s22s22p43s1

1s22s22p43s2

Part A. How many grams of NH3 can be produced from 4.78 mol of N2 and excess H2.

Part B. How many grams of H2 are needed to produce 10.52 g of NH3?

Part C. How many molecules (not moles) of NH3 are produced from 5.64×10⁻⁴ g of H2?

Avogadro’s Law. Now imagine that you open the jar and pull the balloon out. Now imagine that you put 3.00 g of the same gas in another balloon at the same pressure and temperature. (a) The volume of the second balloon is _____ times _______________than the volume of the first balloon at the same conditions. In this experiment (pressure/temperature/amount) (is/are) constant. (b) Calculate the new volume using the ideal gas law. (c) Now explain the change in volume from behavior of the gas molecules.

Q1/50 grams of an unknown metal at a temperature of 100 ºC is placed in a calorimeter that holds 25.0 grams of cold water (10 ºC). After 10 minutes, the temperature of the mixture stabilizes at 24 ºC. What is the specific heat capacity of the unknown metal? (Specific heat of water is 4.184 J  g 1  C1 ) a. 0.496 J d. 0.335 J b. 0.421 J e. 0.689 J c. 0.385 J

the answer is B 0.421 J but i dont know how?

Q2/ How many grams of methane must be burned to produce 1000 kJ of energy, according to the following reaction:: CH4  2O2 CO2  2H2O H = –890.4 kJ a. 90 g d. 18 g b. 9 g e. 38 g

The answer is D 18g but i dont know how

Would your calculated percent NaNo2 by mass by larger than, smaller than or unchanged from the correct value as a result of the following mistakes? Show your reasoning or calculations when appropriate.

A) You neglected to open the stopcock on your buret prior to the evolution of nitrogen gas.

B) Your measured temperature was erroneously recorded 5 degrees C higher than actual temperature.

C) You neglected to correct for the vapor pressure of water in your calculations.

3. Chemical reactions and equilibrium constants

(a) An alternative way of writing the reaction for the dissolution of CdCO3(s) is to form the species HCO3- rather than CO32-.
Write a balanced chemical reaction for CdCO3(s) dissolution with HCO3- rather than CO32- as a product species.
Calculate an equilibrium constant and standard free energy of reaction for your new reaction. You will need to look up some equilibrium constants.

(b) How would you decide which reaction to use to describe the equilibrium of CdCO3(s) with water? From the standpoint of chemical equilibrium, does it matter? Explain.

Indicate which vibrational modes will be IR-active and Raman-active. Briefly explain.

Acetylene, symmetric triple bond stretch

Benzene, symmetric ring CC stretch

Carbon dioxide, asymmetric C=O stretch

trans 1,2 dibromoethene, sym C=C

SO3(g) can be produced by this two step process:

1.) 2FeS2 + 1 1/2 O2 = Fe2O3 + 4SO2

2.) SO2 + 1/2 O2 = So3

How many grams of SO3 can be produced from the reaction of 45.0 g of FeS2 if there is no experimental error? How many grams would actually be measured if reaction 1 had 100% yield and reaction 2 had 83.4% yield?

Predict whether aqueous solutions of the salts will be acidic, basic or neutral. Please explain why, so that I can learn the mechanism. Thank you!

Acidic Basic Neutral  (CH₃)₂NH₂NO₃
Acidic Basic Neutral  C₆H₅NH₃Br
Acidic Basic Neutral  CaBr₂
Acidic Basic Neutral  CsF₃CCOO
Acidic Basic Neutral  Cs(NO₃)

Part A

Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the pH. What was the Ka value calculated by the student if the pH of the solution was 2.62?

Part B

A 0.100 M solution of ethylamine (C2H5NH2) has a pH of 11.87. Calculate the Kb for ethylamine.

LAB Reaction Rates

Objectives

• Evaluate the effect of concentration on the rate of a chemical reaction. ν

• Examine the effect of temperature on the rate of a chemical reaction.

Background: Many people believe that you cannot perform chemical reactions without expensive equipment or costly chemicals. But this isn’t true; chemical reactions happen everywhere. All you need is a food store to find many substances that can produce exciting chemical reactions.

Preparation

Materials

water	vinegar solution
baking soda	balloons (3)
plastic 0.5-liter	test tube
soft-drink bottles (3)	150-mL beakers (2)
marker	500-mL beaker
stopwatch, or clock	100-mL graduated
with second hand	cylinder
tape

Safety Precautions

Procedure

1. Read the procedure and safety information, and complete the lab form.

2. Make data tables similar to those shown on the next page.

3. Prepare a 50 percent vinegar solution by mixing 30 mL of vinegar with 30 mL of water. This is solution A.

4. Prepare a 30 percent vinegar solution by mixing 30 mL of vinegar with 70 mL of water. This is solution B.

5. Prepare a 10 percent vinegar solution by mixing 30 mL of vinegar with 270 mL of water. This is solution C.

6. Pour the vinegar solutions into their associated 0.5-L plastic bottles labeled A, B, and C.

7. Mark a small test tube about 1–2 cm from its bottom. Fill the test tube to the line with baking soda. Pour the baking soda into one balloon.

8. Repeat step 7 with two more balloons. Be sure the amount of baking soda in each balloon is the same.

9. Place the mouth of one balloon over the mouth of one 0.5-L bottle. Do not let any of baking soda fall into the vinegar solution.

10. Repeat step 9 with the other two balloons and the remaining bottles.

Inquiry Lab

11. Lift each balloon to allow the baking soda to fall into each vinegar solution. Time how long it takes for the reaction to finish. Measure how much each balloon inflates. Record your observations in your Concentration data table.

12. Carefully remove the balloons from the bottles.

13. Rinse the plastic bottles with water.

14. Prepare a 30 percent vinegar solution by mixing

30 mL of vinegar with 70 mL of cold water.

15. Prepare two more similar solutions with room-temperature water and hot water.

16. Place the three solutions in the three 0.5-L plastic bottles.
17. Repeat steps 7 and 8 to refill the balloons with baking soda.

18. Place the balloons back on the bottles, repeating steps 9 and 10.

19. Repeat step 11. Time how long it takes for the reaction to finish.

20. Measure how much each balloon inflates. Record your observations in your Temperature data table.

Concentration Data Table (Ballon circumferrence)

Vinegar Concentration	Solution A (50%)	Solution B (30%)	Solution C (10%)
Observations	8.5 cm	6.20cm	4.00cm

Temperature Data Table (Circumferrence of ballon)

Solution temperature	Cold Room Temperature	Room Temperature	Hot temperature
Observations	3.50 cm	5.00 cm	7.00 cm

Analyze Your Data

1. Describe how increasing the concentration of a solution affects the rate of a chemical reaction. (Concentration increases rate increases)

2. Summarize how temperature affects the rate of a chemical reaction.(Temperature increases rate increases)

3. Explain why the balloons become inflated.( Because of Co2)

Conclude and Apply

4. Infer why the vinegar solutions in steps 3, 4, and 5 were different volumes. Why couldn’t the volumes be the same?

5. Predict what factors might affect the amount of product that is produced. What factors affect the rate at which products are produced?

a 4.4766g sample of petroleum product was burned in a tube furnace, and the SO2 produced was collected in 3% H202. reaction:

SO2 + H2O2 -> H2SO4

A 25ml portion of 0.00923 M NaOH was introduced into the solution of H2SO4 , following which the excess base was back-tirated with 13 33ml of 0.01007 M HCl. calculate the ppm of sulfur in the sample

Use what you learned about [H3O(+)] and pH formulas to solve the following problem

Calculate the pH of a (1.99x10^-1) M solution of Na2S03 (Kb1 = 1.56E-7, Kb2 = 5.88E-13)

1. Carbon monoxide (CO) normally binds tightly to heme (aq). How is this decreased in Mb? What are the relative CO vs. O2 binding strengths in each case?

2. Explain the role of BPG in Hb function. How is BPG involved with adaptation to high altitude? Draw and label a graph that illustrates Hb at low and high altitude.