
The density of palladium (Pd) is 12.0 g/mL and the cell volume is 5.89 ✕ 10^−23 mL. Determine the number of atoms in the unit cell. (Because there cannot be a part of an atom in a unit cell, we must round the number of atoms to the nearest whole

The element palladium has ccp packing with a facecentered cubic unit cell. The density of Pd is 12 g/cm3. Calculate the volume (L) of the unit cell of Pd.

1)The element nickel has ccp packing with a facecentered cubic unit cell. The density of nickel is 8900 kg/m3 and the cell volume is 4.376 x 1023 cm3. Calculate the value of Avogadro's number to three significant figures based on these data. (Note: the

The unit cell of palladiu m is a cube that is 389. 03 pm on a side. There are 4 Pd ato ms in the unit cell. Calculate the density of palladium in grams per cubic centimeter.

The metal palladium crystallizes in a facecentered cubic lattice with an edge length of 388.8 pm. What is the density of the palladium?


The density of gold is 1.93E4 kg/m3 and the cell volume is 6.78E26 L. Determine the number of atoms in the unit cell. Note: the number of atoms in a unit cell is a whole number. For the purposes of this calculation, enter your answer to 3 significant

The density of iridium is 22400 kg/m3 and the cell volume is 5.66 x 1023 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

The density of platinum is 21500 kg/m3 and the cell volume is 6.04 x 1026 L. Determine the number of atoms in the unit cell. Note: the number of atoms in a unit cell is a whole number.

The density of cesium is 1870 kg/m3 and the cell volume is 2.23 x 1022 mL. Determine the number of atoms in the unit cell. Note: the number of atoms in a unit cell is a whole number.

1.The density of solid Fe is 7.87 g/cm3. What volume per atom of Fe? 2.As a solid Fe adopts a body centered cubic unit cell. What is the volume of a unit cell of this metal? 3.What is the edge length of a unit cell of Fe?

How would i calculate the density of Li2S in grams per cubic centimeter? I have to use the equation : density= mass/ volume: But i don't know how to find out the volume using the edge length of the unit cell which is 5.88* 10^2 pm.

Based on the number of atoms per unit cell and the mass of the atom, the mass of the unit cell can be calculated. The density of the unit cell and the material as a whole can be determined from the mass and the volume of the unit cell as. D= M/V The usual

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

The proteins in a mammalian cell account for 18% of its net weight. If the density of a typical mammalian cell is about 1.1 g/mL, and the volume of the cell is 4x109 mL, what is the concentration of protein in mg/mL?

1) mass=100g, volume=10ml,density= 2) volume=7ml, mass=70g, density= 3) mass=50g, volume=10cm3, density= 4) volume=30cm3,mas=90g,density= 5) mass=120,volume=6ml,density= Thanks everyone i apresheate your help.


1) mass=100g, volume=10ml,density= 2) volume=7ml, mass=70g, density= 3) mass=50g, volume=10cm3, density= 4) volume=30cm3,mas=90g,density= 5) mass=120,volume=6ml,density= Thanks everyone i apresheate your help.

Although these quantities vary from one type of cell to another, a cell can be 2.10 ìm in diameter with a cell wall 50.3nm thick. If the density (mass divided by volume) of the wall material is the same as that of pure water, what is the mass (in mg) of

can anybody give me the density of arsenic oxide at STP is this the correct formula volume = mass/ density thanks Yes, but if you want the density, it is density = mass/volume. The number I have seen floating around on this board is 17.8 g/L but the

Hydrogen gas dissolves in palladium with the hydrogen molecules going into the spaces between the metal ions. Determine the molarity, molality, and percent by mass of the H2:Pd solution (d=10.8g/cm)containing 0.94g hydrogen gas dissolved in 215 grams of

Please help !!! A student wanted to determine the density of an object made of an unknown substance. She found the mass of the object was 335g. Then she did water displacement to determine the objects volume. The initial volume of the water was 50.0 mL.

An element has bcc packing with a bodycentered cubic unit cell. Its density is 19300 kg/m3 and the unit cell volume is 3.17 x 1026 L. Calculate the molar mass (g/mol) of the element to three significant figures. The element rubidium has bcc packing with

 What fraction of an E coli cell is occupied by its DNA? How would I find the fraction? If I knew the volume of an E coli cell, would I divide that by the volume of DNA in an E coli cell?  A human cell is typically spherical with a diameter of 20

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

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 element Sc has hcp packing with a hexagonal unit cell. The density of Sc is 3000 kg/m3. Calculate the volume (L) of the unit cell of Sc. Sc Molar Mass =44.956 It is hcp, so it has 2 atoms/unit cell. I would appreciate any help with this problem! Thank


1. The element gold, Au, has a facecentered cubic structure. (Density  19.3 g/cm^3) (a) What are the # of gold atoms in 1 unit cell? (b) What are the # of unit cells in 1 mol? (c) What is the volume of 1 mol gold unit cells? (d) What is the volume of 1

1. The eleent gold, Au, has a facecentered cubic structure. (Density  19.3 g/cm^3) (a) What are the # of gold atoms in 1 unit cell? (b) What are the # of unit cells in 1 mol? (c) What is the volume of 1 mol gold unit cells? (d) What is the volume of 1

Initial info: The atoms of crystalline solid pack together into a threedimensional array of many small repeating units called unit cells. The simplest of the unit cells are those that have cubic symmetry, with atoms positioned at the corners of a cube.

Gallium crystallizes in a simple cubic lattice. Sketch the unit cell. Determine the number of atoms present in the unit cell. The density of gallium is 5.904g/cm^3. Determine a value for the atomic (metallic) radius of gallium.

I have a unit cube question to which the answer is given that I'm trying to figure out. The question is: If under conditions of high pressure & temperature, the crystalline structure rearranges to form a facecentered cubic unit cell, what is the new

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

The element Xe has ccp packing with a facecentered cubic unit cell. The density of xenon is 3.783 g/mL and the cell volume is 2.306 x 1022 mL. Calculate the value of Avogadro's number to three significant figures based on these data.

The element Rb has bcc packing with a bodycentered cubic unit cell. The density of Rb is 1.532 g/cm3 and the cell volume is 1.852 x 1022 mL. Calculate the value of Avogadro's number to three significant figures based on these data.

A particular object weighs 313 N in air and 264 N when immersed in alcohol of density 0.70 g/cm3. What is the volume (in L) and the density (in kg/m3) of the object? I had origionally used the 264N as the force of buoyancy and did the Fb=density*volume*g,

The element rubidium has bcc packing with a bodycentered 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


The element Sc has hcp packing with a hexagonal unit cell. The density of scandium is 3.00E3 kg/m3 and the cell volume is 5.00E26 L. Calculate the value of Avogadro's number to 3 significant figures based on these data. Note: the value may differ from the

Titanium metal has a bodycentered cubic unit cell. The density of Titanium is 4.50 g/cm^3. Calculate the edge length of the unit cell and a value for the atomic radius of titanium. Ok, I know how to find the density using the atomic radius, but I'm having

A voltaic cell is constructed that uses the following halfcell reactions. Cu+(aq) + e Cu(s) I2(s) + 2 e 2 I (aq) The cell is operated at 298 K with [Cu+ ] = 2.3 M and [I  ] = 3.3 M. (a) Determine E for the cell at these concentrations. (b) If [Cu+ ]

A voltaic cell is constructed that uses the following halfcell reactions. Cu+(aq) + e Cu(s) I2(s) + 2 e 2 I (aq) The cell is operated at 298 K with [Cu+ ] = 2.3 M and [I  ] = 3.3 M. (a) Determine E for the cell at these concentrations. (b) If [Cu+ ]

For this activity, we had to make cube shaped models to represent cells. Then we had to compare aurafve area, volume, and surface area to volume ratio (SA:V) between the cells. Cell A: length of one side=1cm Surface area= 6cm^2 Volume= 1cm^3 SA:V= 6 Cell

For this activity, we had to make cube shaped models to represent cells. Then we had to compare surface area, volume, and surface area to volume ratio (SA:V) between the cells. Cell A: length of one side=1cm Surface area= 6cm^2 Volume= 1cm^3

For the reaction that occurs in the voltaic cell Fe(s)Fe2+(aq)Cr3+(aq),Cr2+(aq)Pt(s) use data from Appendix D in the textbook to answer the following questions: a)Determine the equation for the cell reaction b)Determine E0 cell c)Determine ΔG0

One gram of palladium has 5.66×10^21 atoms, and each palladium atom has 46 electrons. How many electrons are contained in 7.00g of palladium? The elemental charge is1.6×10^−19C. Answer in units of electrons. The answer is 1.82252x10^24 for Part A.

REALLY NEED HELP WITH THIS PLEASE. One gram of palladium has 5.66×10^21 atoms, and each palladium atom has 46 electrons. How many electrons are contained in 7.00g of palladium? The elemental charge is1.6×10^−19C. Answer in units of electrons. The

One gram of palladium has 5.66×10^21 atoms, and each palladium atom has 46 electrons. How many electrons are contained in 7.00g of palladium? The elemental charge is1.6×10^−19C. Answer in units of electrons. The answer is 1.82252x10^24 for Part A.


a)Calculate the lattice constant a in palladium (Pd).express your answer in angstroms. b) Calculate the distance (in angstroms) between adjacent (110) planes in palladium (Pd). Hint: use your work from part (a).

To determine the density of block of aluminum, you measured the mass at 101.1 g and a volume of 38.2 cm3 . When you looked up the value for aluminum density you found out it should be 2700 kg/m3 What is the percent error for your experimental data? a)

The element strontium has ccp packing with a facecentered cubic unit cell. The volume of the unit cell is 2.25 x 1025 L. Calculate the density (g/mL) of the element.

The element lithium has bcc packing with a bodycentered cubic unit cell. The volume of the unit cell is 4.32 x 1026 L. Calculate the density (g/cm3) of the element.

The element niobium has bcc packing with a bodycentered cubic unit cell. The volume of the unit cell is 3.59 x 1026 L. Calculate the density (g/cm3) of the element

The halflife of Palladium100 is 4 days. A lab is working with a sample of with 3250mg. Write a function, f(x), to represent the amount of Palladium100 left after x days

An element has hcp packing with a hexagonal unit cell. Its density is 4.5 g/cm3 and the unit cell volume is 3.53 x 1023 mL. Calculate the molar mass (g/mol) of the element to three significant figures.

An element has hcp packing with a hexagonal unit cell. Its density is 21000 kg/m3 and the unit cell volume is 2.94 x 1023 mL. Calculate the molar mass (g/mol) of the element to three significant figures.

An element has hcp packing with a hexagonal unit cell. the volume of the unit cell is 5.71E26 L. Calculate the density (kg/m3) of the element.

An element has ccp packing with a facecentered cubic unit cell. Its density is 1770 kg/m3 and the unit cell volume is 1.50 x 1028 m3. Calculate the molar mass (g/mol) of the element to three significant figures.


An element has ccp packing with a facecentered cubic unit cell. Its density is 8.92 g/cm3 and the unit cell volume is 4.72 x 1026 L. Calculate the molar mass (g/mol) of the element to three significant figures.

An element has ccp packing with a facecentered cubic unit cell. Its density is 8.92 g/cm3 and the unit cell volume is 4.72 x 1026 L. Calculate the molar mass (g/mol) of the element to three significant figures.

(a) Calculate the lattice constant a in palladium (Pd). Use only the information available in the class Periodic Table, and express your answer in angstroms. (b) Calculate the distance (in angstroms) between adjacent (110) planes in palladium (Pd). Hint:

An element has ccp packing with a facecentered cubic unit cell. Its density is 12400 kg/m3 and the unit cell volume is 5.50 x 1029 m3. Calculate the molar mass (g/mol) of the element to three significant figures. Please explain how you come to the

1. Which of the following is an example of density? (1 point) ice floating on top of a river convection currents that cause wind oil spill cleanup all of the above 2. What type of property is density? (1 point) chemical property sizeindependent physical

1)The element nickel has ccp packing with a facecentered cubic unit cell. The density of nickel is 8900 kg/m3 and the cell volume is 4.376 x 1023 cm3. Calculate the value of Avogadro's number to three significant figures based on these data. (Note: the

Palladium crystallizes with a facecentered cubic structure. It has a density of 12.0 , a radius of 138 , and a molar mass of 106.42. What is Avogardo's number?

Sketch one face of a simple cubic unit cell of side a for the case when the maximum fraction of the lattice in volume is filled with atoms, and each atom is approximated by a hard sphere. (ii) What is the radius of each atom in terms of a? (iii) What is

Sketch one face of a simple cubic unit cell of side a for the case when the maximum fraction of the lattice in volume is filled with atoms, and each atom is approximated by a hard sphere. (ii) What is the radius of each atom in terms of a? (iii) What is

I posted this up yesterday: I have to use the equation : density= mass/ volume: But i don't know how to find out the volume using the edge length of the unit cell which is 5.88* 10^2 pm. CHemistry....Please help  DrBob222, Sunday, January 25, 2009 at


Felipe made a toy boat out of clay, but it kept sinking in water. He changed the boat's design by making it slightly wider than before. Why did Felipe's newly designed boat float on water? A. He decreased the density by increasing the volume. B. He

mass of an unknown sample is 0.240 kg in air and 0.208 kg when in oil of density=800 kg/m^3. Determine volume and density. Is the density 0.240/800?

mass of an unknown sample is 0.240 kg in air and 0.208 kg when in oil of density=800 kg/m^3. Determine volume and density. Is the density 0.240/800?

The current research project involves examining the photoreceptors of the fruit fly, Drosophila Melanogaster. Over the last 6 weeks, I have been spending about 2 hours a week working with a program called ImageJ and various slices of photoreceptor cells of

Use these data to estimate Avogadro's number. Palladium crystallizes with a facecentered cubic structure. It has a density of 12.0g/cm^3 , a radius of 138 pm , and a molar mass of 106.42 g/mol .

Palladium crystallizes with a facecentered cubic structure. It has a density of 12.0 g/cm^3, a radius of 138 pm, and a molar mass of 106.42 g/mol. Use these data to estimate Avogadro's number.

The density of solid W is 19.3 g/cm3. How many atoms are present per cubic centimeter of W? As a solid, W adopts a bodycentered cubic unit cell. How many unit cells are present per cubic centimeter of W? What is the volume of a unit cell of this metal?

The current research project involves examining the photoreceptors of the fruit fly, Drosophila Melanogaster. Over the last 6 weeks, I have been spending about 2 hours a week working with a program called ImageJ and various slices of photoreceptor cells of

At 20 degrees C ethanol has a density of 0.789 g/ml and H2O has a density of 1.0 g/ml. What is the % by volume of ethanol of a solution made by adding 50g of ethanol with 50g of H2O? Tutor Answer: Use density = mass x volume to convert 50 g ethanol to

If a block could be molded into a flatter and longer shape, then which one would happen and can you explain? a. mass, volume, and density all would change. b. volume would change, but the mass and density would remaine the same. c. mass and volume would


Using Dimensional analysis, how do you set up a problem to find the density when given mass and volume? Suppose the mass of an object is 40 grams and the volume is 20 mL. Density has units of grams/mL. Then density = 40 g/20 mL = 2 g/mL. If this isn't

this is a wiley plus problem and there is no reading lesson with this section so im not sure how to approach this question: The element iridium has ccp packing with a facecentered cubic unit cell. The density of Ir is 22400 kg/m3. Calculate the volume

The element platinum has ccp packing with a facecentered cubic unit cell. The density of platinum is 21.5 g/cm3. Calculate the volume (cm3) of the unit cell of platinum.

When a crown of mass 14.7 kg is submerged in water, an accurate scale reads only 13.4 kg. Is the crown made of real gold? Ok How do I do this problem I set up my free body diagram Net Force = ma = 0= Ft + Fb  Fg were Ft is the force of tension on the

The DNA of an E coli cell measures 1.4 mm in length, when extended and 20 angstroms in diameter. a) Calculate the volume of DNA in an E coli cell in cm^3 b) What fraction of an E coli cell is occupied by its DNA? c) A human cell is typically spherical with

A voltaic cell is constructed that uses the following halfcell reactions. Cu+(aq) + e− > Cu(s) I2(s) + 2 e− > 2 I−(aq) The cell is operated at 298 K with [Cu+ ] = 2.7 M and [I− ] = 2.7 M. (a) Determine E for the cell at

A voltaic cell is constructed that uses the following halfcell reactions. Cu+(aq) + e− > Cu(s) I2(s) + 2 e− > 2 I−(aq) The cell is operated at 298 K with [Cu+ ] = 2.7 M and [I− ] = 2.7 M. (a) Determine E for the cell at

The nucleus of a hydrogen atom is a single proton, which has a radius of about 1.0 1015 m. The single electron in a hydrogen atom normally orbits the nucleus at a distance of 5.3 1011 m. What is the ratio of the density of the hydrogen nucleus to the

Copper has a unit cell volume of (47.453 A^3) and a face centered unit cell. How would I go about finding the volume of atoms within the unit cell? Would you use Avogadro's # somehow?

An element has ccp packing with a facecentered cubic unit cell. Its density is 1540 kg/m3 and the unit cell volume is 1.73 x 1022 cm3. Calculate the molar mass (g/mol) of the element to three significant figures. CCP: cubic close pack


Thank you Ann! I had the equations and really was closing in on the answer... (stopping for 23 s is what really got me confused) in either case, the displacement for a) is 888 m ! Now I'll try to calculate (b). Thank you much! P.S. This is in response to

Density of a metal cube of dimension 10 inches X 10 inches x 10 inches is 8.05g/cm3. What is its mass? 10inches? isnt that 25 cm? So get the volume in cm^3 by multiplying the three dimensions in cm. Multipy that volume by density. Mass= density*volume

When a block of volume 1.00 × 10–3 m3 is hung from a spring scale, the scale reads 10.0 N. When the same block is then placed in an unknown liquid, it floats with 2/3 of its volume submerged. The density of water is 1.00 × 103 kg/m^3. Determine the

You decide to repeat Archimedes experiment and determine the density of a candle holder. you suspend it from a spring scale and scale reads 8.0N. You then lower the holder into a tub of water until completely submerged and it reads 5.0N. what is the volume

1) Assume that the reference halfcell is changed to a standard mercurymercury (II) halfcell. a) What would be the reduction potential of a standard chlorine halfcell. c) What would be the cell potential of a standard chlorinenickel cell. 2) For each

1) Assume that the reference halfcell is changed to a standard mercurymercury (II) halfcell. a) What would be the reduction potential of a standard chlorine halfcell. c) What would be the cell potential of a standard chlorinenickel cell. 2) For each

suppose you have samples of two metals,A and B. Use the data below to determine which sample occupies the largest volume.. A> mass 25g density 10 g/ml B> mass 65g density 4.0 g/ml

The crystal structure of lithium sulfide (Li2S) is pictured here. The length of the unit cell is 5.88 x 10^2. For this structure, determine: a)the coordination number of Li and S b) the number of formula nunits in the unit cell c) the density of Li2S

A chemist needs 2.00 grams of a liquid compound with a density of 0.785 g/cm^3 density. what volume of compund is required? Mass= Volume X Density 2.00g x 0.785 g/Cm^3 = 1.57g/cm^3 Not sure is this is correct......

Felipe made a toy boat out of clay, but it kept sinking in water. He changed the boat's design by making it slightly wider than before. Why did Felipe's newly designed boat float on water? A. He decreased the density by increasing the volume. B. He


Felipe made a toy boat out of clay, but it kept sinking in water. He changed the boat's design by making it slightly wider than before. Why did Felipe's newly designed boat float on water? A. He decreased the density by increasing the volume. B. He

Felipe made a toy boat out of clay, but it kept sinking in water. He changed the boat's design by making it slightly wider than before. Why did Felipe's newly designed boat float on water? A. He decreased the density by increasing the volume. B. He

Magnesium crstallizes in the hcp arrangment. The dimensions of the unit cell are height 520om, length on an edge, 320. Calculate the density of Mg (s) and compare it with the measured value of 1.738 g/cm^3 this is what i did : m= 2* 24.30g/6.022*10^23 =

Felipe made a toy boat out of clay, but it kept sinking in water. He changed the boat's design by making it slightly wider than before. Why did Felipe's newly designed boat float on water? A. He decreased the density by increasing the volume. B. He

Felipe made a toy boat out of clay, but it kept sinking in water. He changed the boat's design by making it slightly wider than before. Why did Felipe's newly designed boat float on water? A. He decreased the density by increasing the volume. B. He