solvinggod

Suppose that you first titrated 25.0 mL of 0.500 M HCL with 0.500M NaOH and then 25.0 mL of 0.500 M of a weark acid HA with 0.500M NaOH.How would the titration curves compare at 10 or 15 ml of NaOH beyond the equivalence points? Explain.

Rank the CF3Br, CF2ClBr, CF2Cl2 in a sequence of increasing ozone-depletion potential and again explain. 

A 49% dextrous solution (49 mg per 100 mL of solution) is given intravenouslySuppose a total of 2.278 L of the solution is given over a 17-hour period. Complete parts (a) through (c) below

A. What is the flow rate in units of ML/hr

B. What is the flow rate of dextrous

FeO (s) + Fe (s) + O2 (g) → Fe2O3 (s)
Given the following table of thermodynamic data,

Substance ΔHf(kJ/mol) S(J/mol-k)

FeO(s) -271.9 60.75

Fe(s) 0 27.15

O₂(g) 0 205

Fe₂O₃(s) -822.16 89.96

determine the temperature (in °C) above which the reaction isnonspontaneous.

Ca (s) + C (s) + 3/2 O2 (g) ---> CaCO3(s)

ΔHrxn = -1207.1 K

---> give ΔHrxn and exothermic or endothermic

a) 2 Ca (s) + C (s) + 3O2 ---> CaCO3 (s)

b) CaCO3 (s) --> Ca (s) + C (s) + 3/2 O2 (g)

c) 2CaCO3 (s) ---> 2 Ca(s) + 2 C (s) + 3O2 (g)

Determine the elastic potential energy stored in a spring with a spring constant of 50 N/m that is compressed 0.29 m

Problem Page

A military jet cruising at an altitude of 12.0kmand speed of 1900./kmh burns fuel at the rate of 74.4/Lmin. How would you calculate the amount of fuel the jet consumes on a 1050.km mission? Set the math up. But don't do any of it. Just leave your answer as a math expression.

Also, be sure your answer includes all the correct unit symbols.

Superfine 40-gauge copper wire has a diameter of only 0.080 mm and weighs only 44.5 g/km. Suppose a spool of 40-gauge wire weighs 659. g less after some wire is pulled off to wind a magnet. How could you calculate how much wire was used?

Set the math up. But don't do any of it. Just leave your answer as a math expression.

Also, be sure your answer includes all the correct unit symbols.

Length of wire = _______

A spool of copper wire has a mass of 4.26 kg. How long is the wire in the spool if the wire has a diameter of 2.2 mm? (The density of copper is 8.96 g/cm3.)

You need to determine the diameter of a piece of copper wire in mm. The wire is 42.66 cm long and weighs 1.049 g. The density of copper is 8.933 g/cm3.

A piece of copper wire is 50ft long and has a dimater of 2.0 mm. Copper has a denisty of 8.92 g/cm³. What is the mass of copper? Express the answer in kg. (1ft = 30.48 cm, 1 cm = 10 mm and Volume is 3.14 x r²x1)

Please explain and help ! :(

Calculate the length of a copper wire having a diameter of 0.200 cm and amass of 15.620 g. The density of copper is 8.92 g/cm3. (Given: volume =??d2 L/4, where ? = 3.14, d = diameter, and L = length)

calculate the length of a copper wire having a diameter of 2.00 cm and a mass of 15.520 g. The density of copper is 8.92 g/cm.

The mass of an empty wooden spool is 45.807 g. The mass of the same spool with a metal wire coiled around it is 66.544 g. Four pieces of wire are cut off from the spool: The length and mass of each piece are as follows: 5.0 cm, 1.401 g; 11.0 cm, 3.083 g; 14.5 cm, 4.063 g; 20.5 cm, 5.745 g. The diameter of the wire is 2.0 mm. All measurements are made at 25

What is the density of lithium metal in g/cm^3 if a cylindrical wire with a diameter of 2.40 mm and a length of 15.0 cm has a mass of 0.3624 g?

A 3.0765 g piece of aluminum wire with a circular cross-section is 34.31 cm long and has a density of 2.6989 g/cm^3

a) Calculate the volume of the wire in cm^3

b) What is the cross-sectional area of the wire in cm^2

c) What is its diameter in mils if 1 mil=10^-3 inches?

1. What is the idea and principles behind AI?

How to learn math?

A toll collector on a highway receives $4 for cars and $5 for buses. At the end of a 2-hour period, she collected $104. How many cars and buses passed through the toll booth during that period? List all possible solutions.

My problem is with SIGNIFICANT FIGURE

COPPER: Copper has a density of 8.96 g/cm^3. An ingot of copperwith a mass of 57 kg (126lb) is drawn into wire with a diameter of9.50 mm. What length of wire (in meters) can be produced? [Volumeof wire = (pi)(radius)^2(length)]


d = 8.96 g/cm^3
m = 57 kg x 1000g/1 kg = 57000 g
dia = 9.50 mm x 1 cm/10mm = 0.95 cm
radius = 0.48 cm

v = m/d
v= 57000 g / 8.96 g/cm^3 = 6361.6 => 6360 cm^3

[Volume of wire = (pi)(radius)^2(length)]
6360 cm^3 = (3.14)(0.48 cm)^2(length)

Length = 6360 cm^3/ 0.72 cm
Length = 8833 cm^2
Convert to meter:
8833 cm^2 x 1m^2/ 10000 cm^2 = .8833 m^2 => .88 m^2

A. What volume (in cm^3) does 5.00 lbs of copper occupy? ( Density of copper= 8.96 g/cm^3 , 1lb=454g)

B. If the diameter of the wire is 1.25 mm, what is the radius in cm?

C. What is the cross sectional area of the wire in cm^2?

D. Determine the length of the wire in cm.

E. Convert your answer from part (d) to feet. (1in 2.54, 1ft= 12 in.)

A 4.5085 g piece of aluminum wire with a circular cross-section is 41.90 cm long and has a density of 2.6989 g/cm3.

a)Calculate the volume of the wire.

b)What is the cross-sectional area of the wire in cm2?

c)What is its diameter in mils if 1 mil = 10–3 inches?

A piece of alloy in the form of a disc weighs 50.0 g. The disc is 0.250 inches thick and has a circular cross-section of diameter 1.380 inches. What is the density of the alloy in grams per cubic centimeter?

1. An object weighing 12.22 g is added to 24.97mL of water in a graduated cylinder. The water level rises to 27.66mL. Calcualte the density of the material?

2. A piece of alloy in the form of a disk weights 50.0 grams. The disc is 0.250 inches thick and has a circular cross-section of diameter 1.380 inches. What is the density of the alloy in grams per cubic centimeter?

3. A wooden block, 10"x10"x2.0" , weights 3 Ib. 6 oz. What is the density of the wood in ounces per square inches?

4. A steel ball has a diameter of 0.750 cm and weights 1.765 g. What is its density in grams per cubic centimeter?

*show steps please!

Accuracy, Precision, & Density Lab

Make sure to show significant figures and units in your work! Problems due next lab.

1-The density of a metal is 4.91 grams per cubic centimeter. What is the mass in kilograms of a cube of this metal that measures 0.650 meters on each side?

2- The density of chloroform is 1.4832 grams per milliliter. How many milliliters would you use if you wanted 120.2 grams of chloroform?

3- A large tanker truck for carrying gasoline has a capacity of 37017 liters. The density of gasoline is 0.670 grams per cubic centimeter. What is the weight, in pounds, of a full load of gasoline?

4- A metal alloy has a density of 8.5 grams per cubic centimeter. What is the volume in cubic inches of 11.50 pounds of the alloy?

5- Calculate the density in grams per cubic centimeter of a block of wood which weights 5.60 kilograms and has dimensions of 25 cm x 10 cm x 50 cm.

The density of solid Cr is 7.15 g/cm3. How many atoms arepresent per cubic centimeter of Cr? in atoms/cm^3

As a solid, Cr adopts a body-centered cubic unit cell. How manyunit cells are present per cubic centimeter of Cr? in unitcells/cm^3

What is the volume of a unit cell of this metal? in cm^3

What is the edge length of a unit cell of Cr? in cm

1.A block of metal has dimensions 5.00 cm x 2.50 cm x 3.00 cm. Calculate the volume of the block, showing the answer to the correct number of significant figures and unit.

2.If the block of metal from question 2 has a mass of 405.3 g, what is the density of the metal? Calculate the density, showing the answer to the correct number of significant figures and correct unit.

3.Convert the numerical value of the density in question 2 from units of grams per cubic centimeter (g / cm3) to milligrams per milliliter (mg / mL). Note:

-there are 1000 milligrams in a gram.

-the volume unit cubic centimeter cm3 equals the milliliter mL.

Keep the new density to the same significant figures as you reported in question 2

4.A finely-powdered white solid is known to be homogeneous mixture rather than a pure substance. A sample of this solid completely dissolves in water. Give TWO possible substances that could make up this solid mixture, and briefly explain your choices.

5.If your percent SALT in Lab 2 is relatively low, it can be assumed that some salt did not go into the filtrate (the liquid that passes through the filter paper), but rather may have been trapped with the sand. Explain briefly how you could recover any of this "missing" salt?

6.A brand of aspirin claims to contain 325 mg (1 g = 1000 mg) of aspirin per tablet. In addition to pure aspirin, a tablet also contains a non-active filler. We assume that the tablet contains only these two components: aspirin and filler. If a single tablet weighs 1.17 g, calculate the percent filler. Hint: calculate percent aspirin FIRST using the formula

% aspirin = [ (mass aspirin ÷ mass tablet) x 100], the find % filler. When using this formula, make sure the masses of aspirin and tablet have the same units.

7.Water has a density of 1.00 g/mL, and chloroform has a density of 1.49 g/mL. These two liquids do not mix with each other, but rather, form two layers when combined.

8.Equal volumes of water and chloroform are placed in a beaker. A piece of nylon is dropped in the beaker, and is seen to float the the interface (the boundary) of the two liquid layers.

Give a possible value for the density of nylon, including the correct units. Explain your answer briefly.

9.A procedure similar to that used in Lab 3 was performed to find the density of cyclohexane, which has an actual density of 0.779 g/mL, Due to poor lab technique, an experimental density of only 0.663 g/mL is found. Calculate the percent error for the density. Give your answer to the correct number of significant figures.

10.Two white powders are given to you. One is pure sodium bicarbonate, and the other is baking powder (a mixture of sodium bicarbonate and a weak acid like citric acid). Which single test (NOT counting the visual examination with a hand lens) used in Lab 3 allows you to distinguish sodium bicarbonate from baking powder? Explain your answers completely.

11.Gold has a specific heat of 0.129 J/g^oC. If a piece of gold (initially at 10.0^oC) is dropped into hot water, the final temperature of both the gold and the water is measured as 70.9^oC. If it is known that 4560 J of heat transferred from the hot water to the gold, what is the mass of the piece of gold in grams? Give your answer to the correct number of significant figures.

12.It is stated in the Introduction to Lab 4 that q_water = -q_metal. This equation means that if a hot piece of metal is placed in water, the amount of heat given off by the metal is exactly equal to the amount of heat absorbed by the water. However, this equation is not always accurate, because not all of the heat from the metal necessarily goes to the water. Where else can some of the heat go if it is not absorbed by the water?

13.A certain brand of breakfast cereal claims to have 100 Calories per 28 gram serving. 150.0 grams of cereal are burned using a procedure similar to that used in Lab 4. How many calories of heat are released? Note 1 food Calorie (capital C) = 1000 heat calories (lower case c)

14.The oxalate anion C2O42- is found in many dark green vegetables, including spinach, swiss chard, and collard greens. When cations react with oxalate, the resulting ionic compounds are insoluble in water except Group I A oxalates (e.g. compounds of lithium, sodium, potassium, etc. and oxalate) and ammonium oxalate (NH4)2C2O4. These exceptions are soluble in water.

15.Spinach leaves are cut into small pieces, mashed with small amounts of boiling water, and filtered through filter paper to remove the insoluble spinach material. The resulting aqueous extract contains the oxalate anion.if a small amount of the spinach extract is mixed with a small amount of a calcium acetate solution, Ca(C2H3O2)2(aq), what do you expect will be observed?

16.If a small amount of the spinach extract from question 16 is mixed with a small amount of a potassium acetate solution, KC₂H₃O₂(aq), what do you expect will be observed?

17.If a hot water extract of another vegetable is mixed with calcium acetate solution and a white precipitate is observed, does this automatically indicate the presence of the oxalate anion in this vegetable? Explain your answer.

The ABC cereal company is developing a new type of breakfastcereal to compete with a rival product that they call brand x. Youare asked to compare the energy content of the two cereals to seeif the new abc product is lower in calories so you burn 1.00-gsamples of the cereals in oxygen in a calorimeter with a heatcapacity of 600. J(C)^-1. When the Brand X cereal sample burned,the temperature rose from 300.2 K to 309.0 K. When the ABC cerealsample burned, the temperature rose from 299.0 K to 307.5 K. (a)What is the heat output of each sample? (b) One serving of eachcereal is 30.0 g. How would you label the packages of the twocereals to indicate the fuel value per 30.0-g servings in joules?in nutritional calories (kilocalories)?

Question 10

Encapsulation and abstraction differ as ____________

◯ Can be used any way

◯ Hiding and Binding respectively

◯ Binding and Hiding respectively

◯ Hiding and hiding respectively

How much does a spring with a spring constant of 400 N/m need to be compressed in order to store 8.5 J of elastic potential energy?

A) On the morning of your exam, you are sitting down at the breakfast table getting ready to have some of your favourite cereal. As you begin eating, you notice that the box says 500 grams and begin wondering "I wonder how many cereal flakes I have put in my bowl."

How would you determine this? Explain the steps you would take to determine how many cereal flakes you have in your bowl.

Aspartame is an artificial sweetener used in many products. The chemical formula for aspartame is C14718/205. Calculate the number of hydrogen atoms in 5 grams of aspartame. Show your work.

Round your final answer to 2 decimal places.

The AM of 9 terms is 15. If one more term is added to this series, then AM becomes 16. The value of the added term is

1) 30

2) 27

3) 25

4) 23

5) 20  

The closer the sample mean is to the population mean,
a. the larger the sampling error
b. the smaller the sampling error
c. the sampling error equals 1
d. None of these alternatives is correct.