answer

watching

views

17 Nov 2019

Can somebody help me fill out part c1 and 2 please

Density Balance no. Solid Unknown Number Tared mass of solid (g) Volume of water (cm^3) Volume of water and solid (cm^3) Volume of solid (cm^3) Density of solid (g/cm^3) Average density of solid (g/cm^3) Liquid Mass of beaker (g) Mass of beaker + liquid (g) Mass of liquid (g) Volume of liquid (mL) Density of liquid (g/mL) Average density of liquid (g/mL) Density of Water Average density of water at room temperature: Circle the questions that have been assigned. Describe what happens to the appearance of a nonluminous flame when the air-control value is slightly closed. Describe what happens to the appearance of luminous flame when the gas-control value is slightly closed. A burning candle produces a luminous flame. What is the fuel for the burning candle? Why is the flame luminous? The solid is not completely submerged in the water. Will this technique error increase, decrease, or have no effect on the reported density of the solid? Explain.

answer

watching

324

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Keith LeannonLv2

15 Nov 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Need help with these questions?? Please help

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 Ã· 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.

Practice Problem Set 1

l. A common approach to calibrate a piece of volumetric glassware is to fill the glassware with water of at a known temperature and then we the water using an analytical balance. The "true" volume e water is then calculated using the density of the water at the recorded temperature. This process is repeated several times to get an average "true" volume of water and an error in the value,

You decide to perform such an experiment on a 10.0 mL volumetric flask, filling the flask to the mark with pure Dl water at 22 C five separate times and then weighing the water added by difference using an analytical balance. You obtain the following results with the analytical balance.

Exp 1 10,0163 g

Exp 2 10.0345 g

Exp 3 10.0558 g

Exp 4 10.0292 g

Exp 5 10.0484 g

Correct these masses for the buoyancy of air (use d 0.0012 g/cm and d 8.0 g/cm and then convert the corrected masses into volumes using the density of water at22 C given in Table 2-7

What is the average volume of water contained in the volumetric glassware and the error (standard deviation) this volume?

Is the glassware marking within the expected tolerance for a Class A volumetric flask?

ls the error reflected in the 5 experimental determinations a reflection of random error or systematic error?

) What is the systematic error revealed in this experiment?

Next you weigh out 0.5516 g of KHP (potassium hydrogen phthalate) and place it in the calibrated 2. 10.0 mL volumetric flask. You then fill the flask to the mark with 30 Cwater and swirl to dissolve the KHP

a) What is the concentration (M) of the resulting KHP solution (remember to correct the mass of KHP or the buoyance of air)?

b) What is the error in the concentration of the KHP solution?

c) Which measurement/device introduces the greatest error to the concentration calculation?

3. You decide to use the solution the next day and upon measuring the temperature of the solution, find that it has decreased to 20 C

a) What is the new concentration (M) of the KHP solution and the error in this value?

b) By how much in percent did the concentration of the KHP solution change from when you made it to when you used it?

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard