# when there is 3.0 x 10^20 molecules in a closed container, the pressure is 1.2 atm. Using a pumper 1.5 x 10^20 more molecules are added to the container. what is the new pressure?

17,190 results
1. ## chem.

A sample of argon at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0. °C. What is the new pressure? 105 atm 45.5 atm 54.9 atm 23.8 atm 42.7 atm

2. ## Chemistry

4NH3+5O2 = 4NO + 6 H20 If a container were to have 10 molecules of O2 and 10 molecules of NH3, initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?

3. ## Chemistry

A gas mixture in a 1.55L at 298K container contains 10.0g Ne and 10.0g Ar. Calculate the partial pressure " in atm" of Ne and Ar in the container

4. ## chemistry

The pressure inside a hydrogen-filled container was 2.10 atm at 21 C . What would the pressure be if the container was heated to 86 C? Pfinal = ?? atm

5. ## physics/chemistry

(a) An ideal gas occupies a volume of 1.0 cm3 at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container. i got that right to be 2.5e19 molecules (b) If the pressure of the 1.0 cm3 volume is reduced to 1.0 10-11 Pa (an

6. ## Chemistry

Container A holds 752 mL of ideal gas at 2.40 atm. Container B holds 179 mL of ideal gas at 4.80 atm. If the gases are allowed to mix together, what is the resulting pressure? Note: Find the partial pressure of each gas in the total volume using a formula

7. ## Chemistry

When solid CO2 (dry ice) is allowed to come to equilibrium in a closed constant volume container at room temperature (300K), 1. the pressure rises until it reaches 1 atm 2. the pressure rises until a liquid-gas equilibrium is reached. 3. the pressure does

8. ## chem

A piece of solid carbon dioxide, with a mass of 6.2 g, is placed in a 4.0 L otherwise empty container at 21°C. ( a) What is the pressure in the container after all the carbon dioxide vaporizes? atm (.86 atm) (b) If 6.2 g solid carbon dioxide were placed

9. ## chem

A spherical glass container of unknown volume contains helium gas at 25°C and 1.950 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 23°C, it is found to have a volume of 1.55 cm3. The gas remaining in the first container shows

10. ## Chemistry URGENT

consider the following container of helium at 45C. intially the valve is closed. After the valve is opened what is the pressure of the helium gas. your start points are 2.00 atm and 9.00L. after opening you have 3.oo atm and 3.00L. The answer is 2.25 atm

11. ## chemistry

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO2(g) NaHCO3(s); ΔH°rxn < 0 Which, if any, of the following actions will decrease the concentration of CO2 gas present at equilibrium? A. lowering the

12. ## Physics

(a) An ideal gas occupies a volume of 1.6-cm3 at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container. (b) If the pressure of the 1.6-cm3 volume is reduced to 1.6 10-11 Pa (an extremely good vacuum) while the

13. ## chemistry

The pressure in a constant-volume gas thermometer is 0.700 atm at 100°C and 0.512 atm at 0°C. (a) What is the temperature when the pressure is 0.0500 atm? °C (b) What is the pressure at 405°C? atm

14. ## Chemistry

At a certain temperature, the Kp for the decomposition of H2S is 0.813. H2S (Two wa arrow) H2(g) + S(g) Initially, only H2S is present at a pressure of 0.280 atm in a closed container. What is the total pressure in the container at equilibrium?

15. ## chemistry

Three gases (8.00 of methane, 18.0 of ethane, and an unknown amount of propane, were added to the same 10.0-L container. At 23.0 C , the total pressure in the container is 3.60 atm. Calculate the partial pressure of each gas in the container.

16. ## Chemistry

Three gases (8.00 of methane,CH4 , 18.0 of ethane,C2H6 , and an unknown amount of propane,C3H8 ) were added to the same 10.0-L container. At 23.0 degress celsius , the total pressure in the container is 3.90 atm. Calculate the partial pressure of each gas

17. ## chemistry

If methane at a pressure of 3.2 atm and at 21 °C is introduced into a container, the gas be heated to ______°C to increase the pressure to 12 atm.

18. ## Chemistry

Nitrogen and hydrogen react to form ammonia. Consider the mixture of N2 and H2 in a closed container. In this container there are 6 diatomic molecules of hydrogen and 6 diatomic molecules of nitrogen. assuming the reaction goes to completion draw a

Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. A)What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behavior.

20. ## chemestry

suppose two gases in a container have a total pressure of 1.20 atm.What is the pressure of gas B if the partical pressure of gas Ais 0.75 atm?

21. ## Chemistry

The partial pressures of the gases in the container are monitored at constant temperature and recorded in the table below. At time t4, is the rate of the reverse reaction greater than, less than, or equal to the rate of the forward reaction? At

22. ## chemistry(total pressure)

Two cylinders at 27C are connected by a closed stopcock ystem. One cyclinder contains 2.4 L of hydrogen gas at o.600 atm; the other cylinder contains 6.8L of helium at 1.40 atm. Assume valve take up no room. what is the total pressure when the valve is

23. ## Chemistry

A closed container is filled with oxygen. The pressure in the container is 435kPa . What is the pressure in millimeters of mercury? (i know that 1atm=760mm Hg=101,325 Pa) How do I use this to solve for the question? so: 435kPa*101,325=44,076,375Pa, & O2 =

24. ## Chemistry

A gas mixture containing N2 and O2 was kept inside a 2 L container at a temperature of 23 C and a total pressure of 1 atm. The partial pressure of oxygen was .722 atm. How many grams of nitrogen were present in the gas mixture?

25. ## Chem

Hello! A 22.0 L cylinder containing helium gas at a pressure of 28.1 atm is used to fill a weather balloon in order to lift equipment into the stratosphere. What is the final pressure (in atm) in the cylinder after a 101 L balloon is filled to a pressure

26. ## chem

A gas at a pressure of 2.0 atm is contained in a closed container. Indicate the changes in its volume when the pressure undergoes the following changes at constant temperature. (Assume that the volume of the container changes with the volume of the gas.)

27. ## chemistry

please can someone help me with these questions? 24) Which represents the largest pressure? A) five mm Hg B) one atmosphere C) one millimeter of mercury D) one hundred pascals E) five pounds per square inch 25) What would be the new pressure if a 400 mL

28. ## chem

at 84 degrees Celsius , a gas in a container exerts a pressure of 0.503 ATM. assuming the size of the container remains the same, at what Celsius temperature would the pressure be 1.20 atm ?

29. ## chem

A spherical glass container of unknown volume contains helium gas at 25°C and 1.950 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 23°C, it is found to have a volume of 1.55 cm3. The gas remaining in the first container shows

30. ## Chemistry

A spherical glass container of unknown volume contains helium gas at 25C and 1.960 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 25C, it is found to have a volume of 1.75 cm^3. The fas remaining in the first container shows a

31. ## chemistry

A piece of solid carbon dioxide, with a mass of 7.4 g, is placed in a 4.0-L otherwise empty container at 27°C. (a) What is the pressure in the container after all the carbon dioxide vaporizes? 1.0atm (b) If 7.4 g solid carbon dioxide were placed in the

32. ## chem

a) Calculate the pressure exerted by 0.5160 mol N2 in a 1.0000 L container at 24.6°C using the ideal gas law. atm (b) Calculate the pressure exerted by 0.5160 mol N2 in a 1.0000 L container at 24.6°C using the van der Waals equation. atm (c) Compare the

33. ## chemistry

A mixture of CH4(g) at 0.500 atm and O2(g) at 0.750 atm is present in a 3.00-L container at 28°C. The mixture is ignited by a spark and reacts according to the equation provided below. What is the total pressure in the container, now at 44°C, after the

34. ## chem

A 75.0 L stainless steel container was charged with 3.00 atm of hydrogen gas and 4.00 atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at 25°C? in atm What is the pressure in the tank at 125°C? in atm

35. ## Chemistry

Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200 oC in a closed container, 1.1 atm of nitrogen gas is mixed with 2.1 atm of hydrogen gas in an otherwise empty container. At equilibrium, the total pressure is 2.2 atm. Calculate

36. ## Chemistry

Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 4.40 atm . Calculate the partial pressure of each gas in the

37. ## chemistry

Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 5.20 atm . Calculate the partial pressure of each gas in the

38. ## Chemistry 105

A sample of nitrogen gas in a 1.86-L container exerts a pressure of 1.32 atm at 20 C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 354 C?

39. ## AP Chemistry

Equal masses of Ne and Ar are placed in a rigid, sealed container. If the total pressure in the container is 1.2 atm, what is the partial pressure of Ar?

40. ## Chm

Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules.What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behavior.

41. ## Chemistry

A rigid container of O2 has a pressure of 3.5 atm at a temperature of 713 K. What temperature would be needed to achieve a pressure of 6.0 atm?

42. ## chemistry

A sample of gas in a closed container at a temperature of 75◦C and a pressure of 6 atm is heated to 353◦C. What pressure does the gas exert at the higher temperature? Answer in units of atm. I got 28.24 and it's wrong A gas has a pressure of 2.92 atm

43. ## chemistry

A container holds 1.00 mol O2, and the pressure in the container is 2.00 atm. A student adds 60.0 g of gas Y to the container. The total pressure (of O2 and gas Y) is 3.00 atm. What is the molar mass of gas Y? (V and T constant)

44. ## chemistry

A closed container with a mixture of hydrogen, helium, and argon has a total pressure of 2.90 atm. The partial pressure of hydrogen is 0.500 atm and the partial pressure of argon is 760. mm Hg. What is the partial pressure of helium?

45. ## Chemistry

A closed container is filled with oxygen. The pressure in the container is 453.97 kPa . What is the pressure in millimeters of mercury?

46. ## cleveland state university

A sample of gas at 1.3 atm of pressure is in a 2.0 L container. What will the pressure be if the sample is transferred to a 0.90 L container? 1. 0.59 atm 2. 1.4 atm 3. 2.9 atm 4. 3.2 atm

47. ## Thermal Physics, Kinetic Theory of Gases

Oxygen (O2) has a molar mass of 32 g/mol. (e) Suppose an oxygen molecule traveling at this speed bounces back and forth between opposite sides of a cubical vessel 0.10 m on a side. Find the average force it exerts on one of the walls of the container.

48. ## Chemistry

Initally, only H2S is present at a pressure of 0.224 bar in a closed container. What is the total pressure in the container at equilibrium? H2S(g)H2(g)+S(g) Initally, only H2S is present at a pressure of 0.224 bar in a closed container. What is the total

49. ## Chemistry

In a fixed volume container, 6*10^23 molecules of a gas exert a pressure of 12 N/m^2. If 12*10^23 molecules of gas were added to the container, what would the pressure become? PV=nRT P=pressure in atm V=volume in L T=absolute (kelvin) temperature R=0.082 L

50. ## Chemistry URGENT/DR BOB

Dalton's Law of Partial Pressure consider the following container of helium at 45C. intially the valve is closed. After the valve is opened what is the pressure of the helium gas. your start points are 2.00 atm and 9.00L. after opening the valve you have

51. ## chem

At a certain temperature, the Kp for the decomposition of H2S is 0.832 H2S (g) H2 (g) + S (g) Initially, only H2S is present at a pressue of 0.121 atm in a closed container. what is the total pressure in the container at equilibrium?

52. ## Chemistry

A container is filled with CO2(g) and heated to 1000K. The gas pressure at this temperature is 0.50 atm. Graphite (C) is then added to the container and some of the CO2 is converted to CO according to the reaction below. The final equilibrium total gas

53. ## physics

An unknown liquid fills a square container of sides 10 m. What is the density of a material if the pressure 5 m below the surface is 1.6 atm? Assume g=10 m/s^2 and the pressure at the surface of the liquid is 1 atm. Also assume that 1 atm = 10^5 Pa. (Hint:

If we believed that the molecules of a gas move around fairly rapidly, we can use this to explain all of the following EXCEPT why adding more gas increases the pressure. why most of the volume of the gas sample is taken up by the gas molecules. why the gas

55. ## chem -help

Two cylinders at 27C are connected by a closed stopcock ystem. One cyclinder contains 2.4 L of hydrogen gas at o.600 atm; the other cylinder contains 6.8L of helium at 1.40 atm. Assume valve take up no room. what is the total pressure when the valve is

56. ## Physics

A container of volume 19.4 cm3 is initially filled with air. The container is then evacuated at 0oC to a pressure of 6.0 mPa. How many molecules are in the container after evacuation if we assume that air is an ideal gas?

57. ## chemistry

You have 120.8 grams of CO2 at 2.5 atm and 18.4oC in a 10.0 L fixed volume container. What is the internal pressure(atm)?

58. ## chemistry

A sample of gas in a closed container at a temperature of 83C and a pressure of 9 atm is heated to 259C. What pressure does the gas exert at the higher temperature? Answer in units of atm

59. ## chemistry

an ideal gas in a closed inflexible container has a pressure of 6 atm and a temperature of 27 degree celsius . What will be the new pressure of the gas of temperature is decreased to -73 degree celsius? a) 2 atm b) 3 atm c) 4atm d) 8atm e) 9atm plz teach

60. ## Chemistry

At a certain temperature, the Kp for the decomposition of H2S is 0.755 H2S (g) H2 (g) + S (g) Initially, only H2S is present at a pressue of 0.201 atm in a closed container. what is the total pressure in the container at equilibrium?

61. ## Chemistry

A closed container with a mixture of hydrogen, helium, and argon has a total pressure of 3.00 atm. The partial pressure of hydrogen is 0.550 atm and the partial pressure of argon is 615 mm Hg. What is the partial pressure of helium?

62. ## chemistry 116

You have a rigid sealed container held at a constant temperature. You add 3.3 atm of oxygen gas, 1.7 atm of nitrogen and 4.2 atm of methane to it. What is the partial pressure of the oxygen gas in the container

63. ## chem

A spherical glass container of unknown volume contains helium gas at 25°C and 1.950 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 23°C, it is found to have a volume of 1.55 cm3. The gas remaining in the first container shows

64. ## chemistry

the pressure in a 1.0 container is 988 ATM what is the pressure in a 2.56L container? ( use gas laws )

65. ## Chemistry

The water from a hydrated magnesium salt is driven off by heat in a closed system. If the steam generated exerts a pressure of 24.8 atm in a 2L container 120 degrees C, determine the number of moles of H2O driven from the compound.

66. ## Chemistry

Use van der Waals’ equation to calculate the pressure exerted by 2.33 mol of ammo- nia at −3.7◦C in a 1.25 L container. The van der Waals’ constants for ammonia are a = 4.00 L2·atm/mol2 and b = 0.0400 L/mol. (The values for a and b have been

67. ## chemistry

Given 1.115 atm of carbon monoxide reactimg with 1.553 atm of oxygen in a closed container at a constant temperatue, what is the theoretic yield of the carbon dioxide?

68. ## Chemistry

A student places 0.025 moles of solid sulfur and 0.100 moles of nitrogen monoxide gas in a closed 1.00L container and 0°c for several days. Calculate the number of molecules of NO in the 1.00L container after equilibrium is reached, given the following

69. ## chemistry

when there is 3.0 x 10^20 molecules in a closed container, the pressure is 1.2 atm. Using a pumper 1.5 x 10^20 more molecules are added to the container. what is the new pressure?

70. ## physics

A closed container with a volume of 8000cm^3 is filled with Xenon gas. the temperature is 273K and the pressure is 2 atm. How many moles of Xenon are in the container? The container is now submerged in boiling water until the gas inside the container is at

71. ## chemistry

At a certain temperature, the Kp for the decomposition of H2S is 0.734.Initially, only H2S is present at a pressure of 0.102 atm in a closed container. What is the total pressure in the container at equilibrium?

72. ## chem 2

At a certain temperature, the Kp for the decomposition of H2S is 0.791. H2S H2 + S Initially, only H2S is present at a pressure of 0.111 atm in a closed container. What is the total pressure in the container at equilibrium? Please Help!

73. ## Chemistry

At a certain temperature, the Kp for the decomposition of H2S is 0.774. H2S(g) H2(g)+S(g) Initially, only H2S is present at a pressure of 0.120 atm in a closed container. What is the total pressure in the container at equilibrium?

74. ## chemistry

an ideal gas in a closed inflexible container has a pressure of 6 atm and a temperature of 27 degree celsius . What will be the new pressure of the gas of temperature is decreased to -73 degree celsius? a) 2 atm b) 3 atm c) 4atm d) 8atm e) 9atm plz teach

75. ## physics

A container of gas with N molecules has the following state variables: P0, V0, and T0. A second container has twice the number of molecules as the first, triple the pressure and T=T0. What is the volume of the second container in terms of V0?

76. ## Chemistry

At a certain temperature, the Kp for the decomposition of H2S is 0.832 H2S (g) H2 (g) + S (g) Initially, only H2S is present at a pressue of 0.121 atm in a closed container. what is the total pressure in the container at equilibrium? Please tell me how to

77. ## Chemistry

At a certain temperature, the Kp for the decomposition of H2S is 0.832 H2S (g) H2 (g) + S (g) Initially, only H2S is present at a pressue of 0.121 atm in a closed container. what is the total pressure in the container at equilibrium? Please tell me how to

78. ## Physics

The lowest pressure attainable using the best available techniques is about 10^-12 N/m^2. At such pressure, how many molecules are there per cm^3 at 0 degrees C. I know that PV= nRT and that you solve for n/v = P/RT. I have also converted from N/m^2 to atm

79. ## chemistry

Consider the conditions listed in the table below. Gas Temperature Pressure H2 100 oC 1 atm CH4 100 oC 20 atm O2 373 K 1 atm CO2 373 K 10 atm Which describes the characteristics of these samples? I. All molecules have the same kinetic energy II. The

80. ## chemistry

A closed container with a mixture of hydrogen, helium, and argon has a total pressure of 2.55 atm. The partial pressure of hydrogen is 0.700 atm and the partial pressure of argon is 705 mm Hg. What is the partial pressure of helium?

81. ## college chemistry

A closed container is filled with oxygen. The pressure in the container is 325 . What is the pressure in millimeters of mercury?

82. ## chemisrty

Q6) A 10 L container contains a mixture of 0.8 g of He and 8 g of Ar at 0 oC. a) (1 pt) Calculate the total pressure of the gas mixture. b) (1 pt) Calculate the partial pressure of each gas in the gas mixture. c) (1 pt) If the initial total pressure of the

83. ## Chemistry

A mixture of 1.39 g H2 and 1.60 g He is placed in a 1.00-L container at 27°C. Calculate the partial pressure of each gas and the total pressure. PH2 = ? atm PHe = ? atm Ptotal = ? atm Please put answer so i can compare to my answer

84. ## Chemistry

Hydrazine, N2H4 can be made (on paper) by reaction of molecular nitrogen and molecular hydrogen, 2 H 2 ( g ) + N 2 ( g ) --> N 2 H 4 ( g ) and suppose that the equilibrium constant Kp has the value 1×10^–3. (a) A stoicheometric mixture of H2 and N2 is

85. ## chemistry

If methane at a pressure of 3.2 atm and at 21 °C is introduced into a container, the gas be heated to ______°C to increase the pressure to 12 atm. is it 352???

86. ## chemistry

we believed that the molecules of a gas move around fairly rapidly, we can use this to explain all of the following EXCEPT why adding more gas increases the pressure. why most of the volume of the gas sample is taken up by the gas molecules. why the gas

87. ## chemistry

the pressure of 3moles of an ideal gas in a container is reduced from 1.0 atm to 0.50 atm against a constant pressure of 0.50 atm at a constant temperature of 273K..what is the change of heat (in J) for the process??Assume that internal energy change at

88. ## chemistry

Suppose two gases in a container have a total pressure of 1.20 atm. What is the pressure of gas B if the partial pressure of gas A is 0.75 atm?

89. ## Chemistry

The water from a hydrated magnesium salt is driven off by heat in a closed system. If the steam generated exerts a pressure of 24.8 atm in a 2.00L container at 120 degrees C, determine the number of moles of H2O driven from the compound.

90. ## physics

A container of volume 14.2 cm3 is initially filled with air. The container is then evacuated at 0oC to a pressure of 32 mPa. How many molecules are in the container after evacuation if we assume that air is an ideal gas?

91. ## St. Martin

A container of volume 20.5 cm3 is initially filled with air. The container is then evacuated at 0oC to a pressure of 19 mPa. How many molecules are in the container after evacuation if we assume that air is an ideal gas?

92. ## Chem

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.

93. ## Chemistry

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.

94. ## chemistry

SO2 and O2 are placed in a 2.00 L container at a temperature of 786 °C and a pressure of 6.99 atm. During the reaction, SO3 forms and the pressure falls to 1.89 atm. Determine how many moles of SO3 are generated.

95. ## Chemistry

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.

96. ## Chemistry

Helium was heated in a sealed container from 18°C to 36°C. The original pressure of helium was 0.84 atm. Find the new pressure assuming V and n remain the same. I put 0.84 over 18 and set it equal to x over 36. I got 1.7 atm but it says its wrong?

97. ## Chemistry

Consider a 980-mL container at 133 °C in which the pressure of nitrogen oxide is 0.394x106 Pa. a) What mass of nitrogen oxide (in g) is present in this container? b) How many molecules is this? (a)----g (b)-----molecules

98. ## chemistry

Nitrogen (N2) and hydrogen (H2) react to form ammonia (NH3). Consider a mixture of six nitrogen molecules and six hydrogen molecules in a closed container. Assuming the reaction goes to completion, what will the final product mixture be? number of NH3

99. ## Attn: DrBob222

A .326L container holds 0.146g of Ne and an unknown amount of Ar at 30C and the total pressure is 627 mmHg. Calculate the moles of Ar present? (I have calculated temp 308K, pressure is 0.825 atm and moles of Ne are .007) Chem - DrBob222, Wednesday, March

100. ## Chemistry

Consider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w = ____ J now calculate the work done if this