--Given Values--
Atomic Radius (nm) = 0.116
FCC Metal = Gold
BCC Metal: = Sodium
Temperature ( C ) = 1017
Metal A = Tin
Equilibrium Number of Vacancies (m^-3) = 6.02E+23
Temperature for Metal A = 369
Metal B = Gallium

I need help with 3, 4, 6, 7, 11, 12. Am I entering the notations incorrectly?

) If the atomic radius of a metal is the value shown above and it has the face-centered cubic crystal structure, calculate the volume of its unit cell in nm³? Write your answers in Engineering Notation.  
        Your Answer =Correct! Exact Answer= 35.3E-3 +/- 1.00E-03%
2) What is the atomic packing factor for the BCC crystal structure?  
        Your Answer = Correct!
3) Find the theoretical density for the FCC Element shown above in g/cm³. Write your answer to the ten thousandths place (0.0000):  
        Your Answer = Incorrect.
4) Calculate the atomic radius, in nm, of the BCC Metal above utilizing the density and the atomic weight provided by examination booklet - Write your answer with 4 significant figures:  
        Your Answer = Incorrect.
5) Calculate the fraction of atom sites that are vacant for copper (Cu) at the temperature provided above. Assume an energy for vacancy formation of 0.90 eV/atom:  
        Your Answer =Correct! Exact Answer= 3.05E-04 +/- 1.00E-05%
6) Repeat the calculation in question 5 at room temperature (25 C):  
        Your Answer = Incorrect.
7) Calculate the energy (in eV/atom) for vacancy formation for the Metal A and the equilibrium number of vacancies at the temperature provided above - Write your answer with 4 significant figures:  
        Your Answer = Incorrect.
8)Calculate the number of atoms per cubic meter in Metal B (units atoms/m³). Write your answer with 4 significant figures :
        Your Answer =Correct! Exact Answer= 5.0961E+28 +/- 1.00E+26%
9) What is the composition, in atom percent, of an alloy that contains a) 36 g Metal A and b) 47 g Metal B? Composition for Metal A (%):  
        Your Answer =Correct! Exact Answer= 31.02769217 +/- 1.00E-01%
10) What is the composition, in atom percent, of an alloy that contains a) 36 g Metal A and b) 47 g Metal B? Composition for Metal B (%):  
        Your Answer =Correct! Exact Answer= 68.97230783 +/- 1.00E-01%
11) What is the composition of Metal A in atom percent, if the alloy consists of 4.5 wt% Metal A and 95.5 wt% of Metal B?  
        Your Answer = Incorrect.
12) What is the composition of Metal B in atom percent, if the alloy consists of 4.5 wt% Metal A and 95.5 wt% of Metal B?  
        Your Answer =

Write a net ionic equations to show how each of hte buffer mixtures below would neutralize added H+ and OH-

a. C6H5COOH and NaC6H5COO H+ + _______ ---> _____________

OH- + _______----> _____________

H+ + ________-----> _____________

b. NH4Cl and NH3 H+ + ________ ------> _____________

OH- + ________-------> ______________

Balance the following redox reaction in basic solution then answer these questions about the balanced reaction. Cl2(g) → Cl-(aq) + ClO-(aq)

Part 1: What is the stoichiometric coefficient in front of Cl2 in the balanced reaction?

Part 2: What is the stoichiometric coefficient in front of OH- in the balanced reaction?

Part 3: What is the stoichiometric coefficient in front of Cl- in the balanced reaction?

Part 4: What is the stoichiometric coefficient in front of OCl- in the balanced reaction?

Part 5: What is the stoichiometric coefficient in front of H2O in the balanced reaction?

Draw a diagram that illustrates the hyperconjugation that explains these phenomena:

- more substituted alkenes have lower heats of hydrogenation

- more substituted carbocations are more stable

- staggered conformations are lower in energy than eclipsed

- allylic SN2 is faster than non-allylic

Be sure to use shading to indicate the location of nodes and use arrows to show overlap.

Thank you!!!

Suppose we are running a Gas Chromatography for a mixture of standard alkanes (C5-C18) in hexane solvent. How do we determine which alkanes are present in the standard from the chromatogram?

Which following molecules expected to be polar? SiBr4 CO2 SO2 BF3

Explain why carbocations are higher in energy than oxonium ions, despite oxygen being more electronegative than carbon. Second, state four factors that account for the relative stabilities of carbocations.

The heme level regulates the globin synthesis because _____.

A sample of gas initially has a volume of 1.42 L at 293 K and 1.30 atm. What volume will the sample have if the pressure changes to 1.50 atm while the temperature is increased to 322 K?

There are a number of steps involved in determining the empirical formula of a compound. You will need to demonstrate that you can complete all of these steps as you determine the empirical formula of a compound composed of phosphorus and chlorine that is 14.87 % P by mass. Complete your calculations based on 100 g of this compound. Enter all calculated values in 4 significant figures followed by one space and the appropriate unit. Use g for grams and mole for moles. Do not use scientific notation.

Determine the mass in grams of chlorine present in the sample. Answer

Determine the number of moles of phosphorus in the sample. Answer

Determine the number of moles of chlorine in the sample.
Answer

The moles of (Answer Cl or P) represents the smaller mole value.

Write the empirical formula of the compound. You will not be able to show subscript values correctly. For example, H2O would be recorded for water.
Answer

3MgCl2(aq) + 2Na3PO4(aq) ------> 6NaCl(aq) + Mg3(PO4)2(s)

1.) If given 29 grams of each reactant, determine the limiting reagent.  

2.) Based on your answer from number 1, what is the theoretical yield of this reaction for Mg3(PO4)2?

3.) Based on your answers from questions 1 and 2, if you were to perform this reaction and generate 20 grams of material, what is the % yield of the reaction?

4.) Based on your answers to the previous 3 questions, when 4 moles of MgCl2 are allowed to react with an excess of Na3PO4 how many moles of NaCl are produced?

1) A certain weak acid, HA, has a Ka value of 4.6×10⁻⁷.

Part A

Calculate the percent ionization of HA in a 0.10 M solution.

Express your answer to two significant figures and include the appropriate units.

1.12×10−2 M Ba(OH)2 Express your answer using three significant figures. Enter your answers numerically separated by a comma.

Part B

Calculate the percent ionization of HA in a 0.010 M solution.

Express your answer to two significant figures, and include the appropriate units.

2)

A 0.120 M solution of a weak acid (HA) has a pHof 3.31.

Calculate the acid ionization constant (Ka) for the acid.

Express your answer using two significant figures.

3)

Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5.

Part A

What is the pH of a 8.00×10⁻²M ammonia solution?

Express your answer numerically to two decimal places.

Part B

What is the percent ionization of ammonia at this concentration?

Express your answer with the appropriate units.

4)

If Kb for NX3 is 8.5×10⁻⁶ , what is the the pKa for the following reaction?

HNX3+(aq)+H2O(l)⇌NX3(aq)+H3O+(aq)

Consider the titration of a 33.0 mL sample of 0.175 M HBr with 0.210 M KOH. Determine each of the following:

Part A the initial pH

Express your answer using three decimal places. pH =

Part B the volume of added base required to reach the equivalence point

Express your answer in milliliters. V =

Part C the pH at 11.0 mL of added base

Express your answer using three decimal places. pH =

Part D the pH at the equivalence point

Express your answer as a whole number. pH =

Part E the pH after adding 5.0 mL of base beyond the equivalence point

Express your answer using two decimal places pH =

How to determine the heat of formation of sucrose after a bomb calorimeter experiment?

A chemistry handbook lists the solubility of sodium iodide (NaL) as 184 g per 100 ml of water at 25^o C.

What would be the percent by mass of a NaL solution prepared by dissolving 95.0 g NaL in 450 g water?