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11 Nov 2019

How many cubic centimeters (cm3 ) of olive oil have the same mass as 1.20 L of gasoline? ​

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Lelia Lubowitz
Lelia LubowitzLv2
21 Jun 2019

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Related questions

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/goC. If a piece of gold (initially at 10.0oC) is dropped into hot water, the final temperature of both the gold and the water is measured as 70.9oC. 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 qwater = -qmetal. 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.

All volume answers should be in the units of Pascals or kiloPascals, all volumes should be in Liters, all temperatures should be in Kelvin, all masses in grams, all densities in g/L, molar masses in g/mol, etc.

1) If I have 5.6 L of a gas in a piston with a pressure of 1.5 atm and compress the gas to 4.8 L, what is the new piston pressure?

2) I have 15 L of air in a balloon at sea level. If I take it to Denver where the air pressure is 85% of sea level, what volume will the air in the balloon take?

3) I have a car with an internal volume of 12000 L. If it goes underwater, it will implode because the air pressure will change from 1.0 atm to 1.4 atm. What would the new volume of the air in the car be?

6) If I have 45 L of helium at 25 °C and increase the temperature to 55 °C what is the new volume?

7) Calcium carbonate decomposes at 1200 °C to form carbon dioxide and calcium oxide. If you collect 25 L of carbon dioxide at 1200 °C, what is the volume of this gas at 25°C.

11) The gas in a can of hairspray has a temp of 27 °C and 30 lbs/in2 of pressure. If the gas reaches a pressure of 90 lbs/in2 the can will explode. What temperature would make that happen?

16) 500 mL of gas at STP. The volume increased to 560 mL and 20 °C, what is the pressure?

17) 400 mL of a gas at 300 mmHg and 0 °C is increased to 10 °C and 140 mmHg, what is the new volume?

18) A balloon has a pressure of 1.05 atm and 5.0 L. If the balloon is released at 20.0 °C but rises to a pressure of 0.65 atm and -15 °C, what is the new volume?

21) What is the partial pressure of carbon dioxide in a container of 5 moles of carbon dioxide, 3 moles of nitrogen gas, and 1 mole of hydrogen gas with a total pressure of 1.05 atm.

26) If neon travels at 400 m/s, what is the velocity of C4H10 at the same temperature?

27) Hydrogen sulfide smells of rotten eggs. C8H8O3 smells of wintergreen. C7H6O smells of almonds. If they are mixed into a container and the container is opened across the room from you, which smell will hit you first?

31) A 50 L container holds 45 moles at 200 °C. What is the pressure?

32) If a 1 L canister holds 2 moles of gas and is thrown into a 1400 °C fire, what is the new pressure in the canister?

36) Calcium carbonate degrades to form carbon dioxide and calcium oxide. How many grams of calcium carbonate are needed to form 3.45 L of carbon dioxide?

37) How many liters of water vapor are formed by combusting 1.25 L of ethene?

41) A gas has a density of 0.53 g/L at 225 K and 108.8 kPa. What is the density at 345 K and 68.3 kPa?

42) 250 mL of a gas at STP weighs 0.291 grams. The composition of the gas is 92.24 % carbon, and 7.76 % hydrogen. What is the gas?

45) The average molar mass of the gases on Titan (a moon of Saturn) is 28.6 g/mol and rests at 95 K and 1.6 atm. What is the density of the gases of Titan?

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