# bcc

45 results

**chemistry**

Is the calculation of percentage of each atom within a Body centered cubic cell AKA volume of the BCC cell same as the atomic packing factor for the BCC unit cell. The BCC % is 68%. the atomic packing factor is just 0.68. Am I completely wrong? And also how do i calculate the ...

**Statistics**

Could someone help out with this question. The answer is 1842, but i'd like to know how to solve it. Thanks BCC wants to estimate the proportion of its students who are single parents. How many students should BCC survey if it wants to be 99% confident that the sample ...

**chemistry**

What is the plane and lattice structure that is represented in this picture? SC (100) BCC (100) FCC (100) SC (110) BCC (110) FCC (110) SC (111) BCC (111) FCC (111)

**Chemistry**

The element rubidium has bcc packing with a body-centered cubic unit cell. The density of Rb is 1530 kg/m3. Calculate the volume (L) of the unit cell of rubidium. Molar mass of Rb=85.468. Since it is bcc, it would have 2 atoms/unit cell. Can you please help me solve this? ...

**Chemistry**

Find the unit cell (simple, bcc, fcc), type of holes where the smaller ions are found (tetrahedral, octrahedral, cubic), and number of cations and anions per unit cell for the following compounds: CdSe CsI Li2O KBr NaCl ZnS(I) i did this and i got most of my answers wrong!!! ...

**bcc**

what are the changes to n02 levels in one day

**Chemistry**

An element has bcc packing with a body-centered cubic unit cell. Its density is 19300 kg/m3 and the unit cell volume is 3.17 x 10-26 L. Calculate the molar mass (g/mol) of the element to three significant figures. The element rubidium has bcc packing with a body-centered cubic...

**bcc**

how do you work equation dealing friction and newtons when pulling the distance of a block

**Physics**

Sodium has bcc packing. If a distance between two nearest atoms is 3.7 A* then what is the lattice parameter?

**Bcc**

suppose x has a mound-shaped distribution with sigma=3. Find the minimal sample size required so that for a 95% confidence interval, the maximal margin of errors is E=0.4

**Science/math**

BCC crystal structure, atomic radius of .1363, and an atomic weight of 95.94g/mol. How would you compute the theoretical density?

**AP chem**

I have a problem set due tomorrow, and two problems in it were not covered in class. The first is this: Molybdenum has an atomic radius of 0.145 nm. The volume of its cubic unit cell is 0.0375 nm^3. What is the geometry of the molybdenum unit cell? I have no idea where to even...

**computers**

In which part of a professional email should you try to be brief, but highly descriptive? A. The subject line B. The blind carbon copy (bcc) C. The emoticons D. The domain I think the Answer is A, is that right?

**math**

an element has a BCC structure with cell edge of 288pm. the density of the element is 7.2g/cm3. how many atom are present in 208g of the element?

**chemistry**

Determine the radius of the largest atom that can be accommodated in the interstices of BCC iron (Fe) without stress. (Hint: the center of the largest site is at ½, ¼, 0; draw a unit cell - it helps.)

**chemistry**

Determine the radius of the largest atom that can be accommodated in the interstices of BCC iron (Fe) without stress. (Hint: the center of the largest site is at ½, ¼, 0; draw a unit cell - it helps.)

**PNU**

An element has a body-centered cubic(bcc) structure with a cell edge of 288pm the density of the element is 7.2g/cm3. How many atoms are present in 208g of element

**chemistry**

The element K has bcc packing with a body-centered cubic unit cell. The density of K is 0.862 g/mL. Calculate the volume (L) of the unit cell of K.

**Biomaterials**

What is the theoretical density of tantalum (Ta) with the following characteristics: Crystal structure: BCC Atomic radius: 14.6 Angstroms Atomic weight: 180.9 g/mol density needs to be in g/cm^3

**chemistry**

The element Rb has bcc packing with a body-centered cubic unit cell. The density of Rb is 1.532 g/cm3 and the cell volume is 1.852 x 10-22 mL. Calculate the value of Avogadro's number to three significant figures based on these data.

**bcc**

if you put honey,water,dishwashing liquid and vegetable oil in a clear jar and then you add asmall of plastic cup, plastic fork, straw and a small piece of styrofoam cup.

**chemistry**

Determine the radius of the largest atom that can be accommodated in the interstices of BCC iron (Fe) without stress. (Hint: the center of the largest site is at ½, ¼, 0; draw a unit cell - it helps.) Radius (in centimeters):

**chemistry**

The element lithium has bcc packing with a body-centered cubic unit cell. The volume of the unit cell is 4.32 x 10-26 L. Calculate the density (g/cm3) of the element.

**Chemistry**

The element niobium has bcc packing with a body-centered cubic unit cell. The volume of the unit cell is 3.59 x 10-26 L. Calculate the density (g/cm3) of the element

**chemistry**

how do i calculate the volume of a unit cell and volume of atoms within a unit cell for FCC and BCC

**algebra**

The number of computers sold by BCC depends on the dollar amound,x, that they spend on advertising. How much must they spend to sell 200 computers? Round to the nearest dollar and do not include units in your answer. N(x)=100+20 * In(0.25x)

**Math Alg2**

The number of computers sold by BCC depends on the dollar amount, x, that they spend on advertising. How many computers will they sell by spending $100,000 on advertising? Round to the nearest whole number and do not include units in your answer.

**Bcc**

suppose x has a mound-shaped distribution. A random sample size 16 has a sample mean of 10 and a sample standard deviation of 2. Find 99% cinfidence interval for mue (mean) using a student's t distribution.

**Math- Alg 2**

The number of computers sold by BCC depends on the dollar amount, x, that they spend on advertising. How many computers will they sell by spending $80,000 on advertising? Round to the nearest whole number and do not include units in your answer. N(x) = 100 + 20 * In(0.25x)

**bcc**

One canned juice drink is 30% orange juice, another is 10% orange juice. How many liters of each should be mixed together in order to get 20L that is 18% orange juice?

**chemistry**

Find the unit cell (simple, bcc, fcc), type of holes where the smaller ions are found (tetrahedral, octrahedral, cubic), and number of cations and anions per unit cell for the following compounds: CdSe CsI Li2O KBr NaCl ZnS(I)

**math**

what is the number of each atom in the unit cell of a BCC cystalline structure unit cell. I know its 2 atoms=8/8 +1 Calculate what % of each atom is contained within the unit cell? How do I do this

**Chemistry**

The density of iridium is 22400 kg/m3 and the cell volume is 5.66 x 10-23 cm3. Determine the number of atoms in the unit cell. Note: the number of atoms in a unit cell is a whole number. The molar mass of iridium is 192.22. I know that this can either be a bcc, cap, or hcp ...

**Chem: x-ray**

Experiment to obtain the X-ray diffraction peaks of an unknown metal. Radiation is K_alpha from Cu. Through these diffraction peaks you wanted to determine: (a) whether the cell is SC, BCC, or FCC (b) the (hkl) value of the peaks (c) the lattice parameter a of the metal sin^2(...

**bcc**

the tail weighed 9 pounds. the hyead weighed as much as the tail plus 1/3 of the body combined, and the body weighed as much as the head and tail combined. what was the total weight of the fish?

**Difracction problem**

Diffraction from an unknown cubic metal is observed to occur at the following values of θ when using CuKα radiation. Determine the crystal structure to find the lattice constant. 20.1⁰, 29.2⁰, 36.6⁰, 43.5⁰, 50.2⁰, 57.4⁰, 65.5⁰...

**Chemistry**

Calculate the radius of a vanadium atom, given that V has a BCC crystal structure, a density of 5.96 g/cm3, and an atomic weight of 50.9 g/mol. I used this equation: density = (2)*(atomic weight) / (volume of unit cell)*(Avagodro's #) rearranged to find the volume of the unit ...

**Chemistry**

Calculate the radius of a vanadium atom, given that V has a BCC crystal structure, a density of 5.96 g/cm3, and an atomic weight of 50.9 g/mol. I used this equation: density = (2)*(atomic weight) / (volume of unit cell)*(Avagodro's #) rearranged to find the volume of the unit ...

**Chemistry**

(a) The phase diagram of the binary system, neodymium-scandium ( Nd-Sc ) is given below. There are two polymorphs in the solid state: alpha which is hexagonal close packed (HCP) and beta which is body-centered cubic (BCC). Identify all phases present at points 1, 2, and 3. ...

**chemistry**

This problem is from my chemistry book and I am having a little trouble with the intermediary steps: Barium metal crystallizes in a body- centered cubic lattice (atoms at lattice points only) The unit cell edge length is 502 pm, and the density of the metal if 3.5g/cm^3. (...

**chemistry**

(a) The phase diagram of the binary system, neodymium-scandium (Nd-Sc) is given below. There are two polymorphs in the solid state: α which is hexagonal close packed (HCP) and β which is body-centered cubic (BCC). Identify all phases present at points 1, 2, and 3. ...

**Chemistry**

DECOMPOSITION OF NO2 (10/10 points) The decomposition of NO2 at room temperature exhibits the following variation in concentration with time: The concentration of NO2 is expressed in mol/liter, while time is expressed in seconds. [NO2] ln[NO2] 1/[NO2] Time (s) 0.0831 -2.4877 ...

**Chemistry**

1- Which of these processes will lower the glass transition temperature of a glass? Increase the cooling rate Decrease the cooling rate Increase amount of network modifier Decrease amount of network modifier Quench the glass to cool the surfaces quickly Decrease the number of ...

**Chemistry**

1- Which of these processes will lower the glass transition temperature of a glass? Increase the cooling rate Decrease the cooling rate Increase amount of network modifier Decrease amount of network modifier Quench the glass to cool the surfaces quickly Decrease the number of ...

**English Check please**

The High School Step Team Karla’s cousin Jade urged her to join the step team. “This afternoon you should definitely try out!” Jade suggested after the final bell rang. “I know she wants the best for me,” Karla thought to herself, “but I’m not sure I’d be any ...

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