Gaseous and liquid states Questions and Answers

A sample of carbon dioxide gas at a pressure of 0.788 atm and a temperature of 22.9 °C, occupies a volume of 546 mL. If the gas is allowed to expand at constant temperature until its pressure is 0.367 atm, the volume of the gas sample will be ___ mL.

A sample of gas contains 0.1600 mol of NH3(g) and 0.2000 mol of O₂(g) and occupies a volume of 20.2 L. The following reaction takes place: 4NH3(g) +50₂(g) ⇒ ANO(g) + 6H₂O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

A sample of neon gas at a pressure of 1.18 atm and a temperature of 26.6 °C, occupies a volume of 15.6 liters. If the gas is compressed at constant temperature to a volume of 7.47 liters, the pressure of the gas sample will be ___ atm.

A 27.3 gram sample of krypton gas has a volume of 942 milliliters at a pressure of 2.04 atm. The temperature of the Kr gas sample is 423.3 °C.

For the following reaction, 3.31 grams of phosphorus (P4) are mixed with excess chlorine gas. The reaction yields 12.0 grams of phosphorus trichloride phosphorus (P4) (s) + chlorine (g) phosphorus trichloride (1) What is the theoretical yield of phosphorus trichloride ? grams What is the percent yield for this reaction? %

Ethylene burns in oxygen to form carbon dioxide and water vapor: C₂H4(g) + 30₂(g) →2CO₂(g) + 2H₂O(g) Under the condition of 1.00 atm and 298 K, how many liters of water can be formed if 4.94 liters of ethylene are consumed in this reaction? Answer with correct significant figures and unit in abbreviation.

The rate of effusion of Xe gas through a porous barrier is observed to be 4.24 x 10 mol/h. Under the same conditions, the rate of effusion of Ne gas would be mol/h.

Ht Values if needed for this question. A sample of krypton gas at a pressure of 0.514 atm and a temperature of 27.4 °C, occupies a volume of 17.1 liters. If the gas is allowed to expand at constant temperature to a volume of 26.3 liters, the pressure of the gas sample will be atm.

A 28.7-g sample of water at 280. K is mixed with 51.8 g water at 350. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. Temperature = K

A sample of gas contains 0.1700 mol of CH4(g) and 0.3400 mol of O₂(g) and occupies a volume of 16.5 L. The following reaction takes place: CH4(g) +202(g)CO₂(g) + 2H₂O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

2.00L of carbon dioxide gas (the main component of the Martian atmosphere) is contained at a pressure of 101.3 kPa at room temperature (21°C) on Earth. The daytime temperature at the equator during summer on Mars is also 21°C. If the atmospheric pressure on Mars is 6.01 mmHg, what volume would the gas occupy on Mars? (3 marks): (A)

The average molecular speed in a sample of N₂ gas at a certain temperature is 515 m/s. The average molecular speed in a sample of Ne gas is 429.05 m/s at the same temperature.

Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H₂O(l) ⇒ 2NaOH(aq) + H₂(g) The product gas, H₂, is collected over water at a temperature of 25 °C and a pressure of 749 mm Hg. If the wet H₂ gas formed occupies a volume of 6.42 L, the number of moles of Na reacted was 1.9407 mol. The vapor pressure of water is 23.8 mm Hg at 25 °C.

Carbon dioxide is collected over water at a temperature of 18°C. The pressure of water vapor at 18°C is 2.20 kPa. If the pressure of the gas collected is 1.05 atm, what is the pressure of the dry gas in kPa? Answer with 1 decimal place and unit in abbreviation. Given: 1.00 atm = 101.3 kPa

If some neon gas at 125 kPa were allowed to change from 11 dm³ to 72 dm³ under constant temperature, what pressure, in kPa, would the neon gas exert under these new conditions? Answer with correct significant figures and unit in abbreviation.

When determining the density of a grape, a student was not careful when putting the grape into the graduated cylinder, and some of the water got splashed out. How would that affect the determined density of the grape? In other words, is the calculated density be higher or lower than the actual density of the grape? Explain your answer (fill in the blanks below). If some of the water got splashed out, the measured "grape + water" volume is incorrectly (high or low?). Then the calculated volume of the grape ("grape+water" - "water only" volume) is incorrectly When calculating the density, the mass is divided by a (higher or lower?) As the result, the determined density is erroneously (high or low?) _ and therefore the determined density is (higher or lower?) than the actual density of the grape.

A sample of oxygen gas has a volume of 150 mL at a pressure of 0.947 kPa. If the temperature remains constant, what will the volume of the gas be at a pressure of 1.000 kPa? P₁V₁ = P₂V₂ Type your work HERE P.,P, are pressure of gas V₁, V, are volume of gas P1= Type Here V1= Type Here P2 = Type Here V2 = Type Here

How many mL of 0.757 M HI are needed to dissolve 8.55 g of MgCO3? 2HI(aq) + MgCO3(s)→→→ MgI₂(aq) + H₂O(1) + CO₂(g) mL

6. A toy balloon containing 425 mL of air escapes from a little boy watching a parade. The temperature is 32°C at street level and the pressure is 745 mm Hg. When a balloon stops rising, its volume has become 895 mL although the atmospheric pressure has decreased by only 300.0 mm Hg. What is the temperature at this level?

The pressure of a sample of gas at 10.0°C increases from 700. mm Hg to 900. mm Hg. What is the new temperature? (Hint: Use Gay-Lussac's Law) 39.0°C 0°C 90.9°C 364°C

The temperature of a 100 mL sample of pure water is 25°C. This is a measure of - A the amount of chemical energy stored in the water molecules B the amount of heat released when water molecules react C the average kinetic energy of the water molecules D the total potential energy of the water molecules

The volume of a sample of oxygen is 300.0 mL when the pressure is 1.00 atm and the temperature is 27.0°C. At what temperature is the volume 1.00 L and the pressure 0.500 atm? (Hint: Use the Combined Gas Law) 22.0°C 45.0°C 0.50 K 227°C

A gas occupies 1.25 L at standard temperature (0 Celsius). What is the volume at 333.0 °C? 1.5L 2.2L 2.8L 31L

The volume of a gas collected when the temperature is 11.0°C and the pressure is 710 mm Hg measures 14.8 mL. What is the calculated volume of the gas at 20.0°C and 740 mm Hg? (Hint: Use the Combined Gas Law) 7.8 mL 14.6 mL 13.7 mL 15 mL

If 15.0 liters of neon at 25.0 °C is allowed to expand to 45.0 liters, what must the new temperature be to maintain constant pressure? 75 C 8.3 C 621 C 1072 C

A sample of oxygen occupies 560. mL when the pressure is 800.00 mm Hg. At constant temperature, what volume does the gas occupy when the pressure decreases to 700.0 mm Hg? (Hint: Use Boyle's Law) 490. mL 80.0 mL 640. mL 600. mL

A balloon has a volume of 2500.0 mL on a day when the temperature is 30.0 °C. If the temperature at night falls to 9.0 °C, what will be the volume of the balloon if the pressure remains constant? 2413 mL 2398 mL 2341 mL 2327 mL

A 600.0 mL sample of nitrogen is warmed from 77.0 °C to 86.0 °C. Find its new volume if the pressure remains constant. 615 ml 623 mL 630 mL 654 mL

Which of the following statements is related to a postulate (assumption) of the kinetic molecular theory of gases? A Gas particles are in constant motion, giving them a large amount of potential energy. B Gas particles are in constant motion so they lose kinetic energy when they collide with the walls of their container. C Gas particles are in constant motion because they are strongly attracted to each other. D Gas particles are in constant motion and are very far apart compared to their size.

The volume of a gas is 50.0 mL at 20.0K. What will be the new temperature if the gas is compressed to 10.0 mL under constant pressure? 100 K 10.0 K 4.00 K 5.00 K

When 50.0 liters of oxygen at 20.0 °C is compressed to 5.00 liters, what must the new temperature be to maintain constant pressure? 0 C -10.34 C -244 C -273 C

P₁/T₁ =P₂/T₂ 10 A sample of a gas in a rigid container at 30.0°C and 2.00 atm has its temperature increased to 40.0°C. What will be the new pressure? A 1.50 atm B 2.67 atm C 2.07 atm D 6.04 atm

What is the new pressure of 80 L of gas that is compressed to 8 L when the original pressure was 3.0 atm and the temperature is held constant? 100 atm 0.90 atm 83.2 atm 30 atm

If the temperature of a gas changes, but the number of moles and volume remain constant, which of the following values must also change? Density Pressure Number of atoms Mass

What is the new pressure of 150 ml of gas that is compressed to 50 ml when the original pressure was 3.0 atm and the temperature is held constant? 100 atm 0.90 atm 1.0 atm 9.0 atm

When the volume of a gas is changed from __ mL to 852 mL, the temperature will change from 315 °C to 452 °C. What is the starting volume? 670 mL 681 mL 685 mL 691 mL

Carbon dioxide is usually formed when gasoline is burned. If 30.0 L of CO₂ is produced at a temperature of 1.00 x 10³ °C and allowed to reach room temperature (25.0 °C) without any pressure changes, what is the new volume of the carbon dioxide?

If I have gas with a volume of 400 mL at a pressure of 2.3 atm and temperature of 21 °C, how many moles of gas do I have?

A 400 mL sample of carbon monoxide is heated from 22 C to 30 C. What will be the new volume? 403 mL 407 mL 408 mL 411 mL

What is the volume of 1 mole of gas at Standard Temperature and Pressure? (STP) 22.4 L 2.4 L 24L 024 L

An open "empty" 2 L plastic pop container, which has an actual inside volume of 2.05 L, is removed from a refrigerator at 5 °C and allowed to warm up to 27 °C. What volume of air measured at 27 °C, will leave the container as it warms? 0.16 L 1.2 L 18L 2.21 L

3.50 liters of a gas at 727.0 C will occupy how many liters at 153.0 C? 1.5L 2.2 L 2.8L 3.9 L

At 27.00 °C a gas has a volume of 5.00 L. What will the volume be at 150.0 °C? 7 L 10 L 12 L 16 L

What are the two characteristic properties of matter? (Select all that apply.) It has mass. It occupies space. It has shape. It can be divided. It has energy.

I have an sample of gas at a pressure of 0.6 atm, volume of 5.8 L and a temperature of 400 K. If I raise the pressure to 1.3 atm and decrease the temperature to 360 K, what will the new volume be? 4. What law are you using to solve this problem? 5. What is the answer to this problem?

Temperature is a measure of: internal energy due to the nuclear interactions between all of the molecules in an object. internal energy due to potential interactions between molecules. total internal energy due to the motions of all the molecules in an object. average kinetic energy of the molecules of a substance.

If the chemist adds HBr gas to a closed chamber with an initial concentration of 1.20 atms, what will the final pressure of H₂ be at equilibrium? Please use the written work page to show your answer and the steps used to find a solution. Submit your Written Work page here.

Vaporization occurs more readily with: A) increased temperature, increased surface area, decreased volume B) increased temperature, increased surface area, increased intramolecular forces C) increased temperature, decreased surface area, decreased intermolecular forces D) increased temperature, increased surface area, decreased intermolecular forces E) decreased temperature, decreased surface area, decreased intermolecular forces

In a certain mountain range, water boils at 93°C. What is the atmospheric pressure under these conditions? The enthalpy of vaporization of water at 100°C is 40.7 J/k . mol (R=8.314 J/K-mol; 1 atm = 760 mmHg) (A) 2040 mmHg (B) 283 mmHg (C) 977 mmHg (D) 278 mmHg (E) 591 mmHg

Solution of water in ethanol form azeotropic mixture when ethanol is 96% by mass. Normal boiling point of C₂H5OH() is 78.6°C and H₂O(t) is 100°C then select correct statements. I. Normal boiling point of azeotropic mixture is 78.7°C. II. If XC₂H5OH = 0.50 then we can obtain only pure H₂O(l) by distillation. III. If XC₂H5OH = 0.98 then we can obtain only pure C₂H5OH by distillation. IV. Normal boiling point of azeotropic composition can be less than 78°C. V. Solution may form minimum boiling azeotropes. I, III, II II, III, IV, V III, IV, V I, II, IV, V