A 7.13 L cylinder contains 1.82 mol of gas A and 3.77 mol of gas B, at a temperature of 31.8 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior. PA= PB = What is the total pressure? PTotal = kPa kPa kPa

Q: A 10.0 L tank at 12.5 °C is filled with 3.91 g of sulfur tetrafluoride gas and 6.79 g of dinitrogen…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 3.91 g Mass of dinitrogen monoxide i.e N2O = 6.79 g…

Q: A gas mixture has partial pressures of 52.55 mmHg H2, 159.74 mmHg N2, and 362.99 mmHg  O2. What is…

A:

Q: Find the mole fraction (in percents) of C2 H2 (g) that has undergone reaction.

A: 3C2H2(g)       ⇔      C6H6 (g) Initial pressure         7.0 kPa…

Q: A 9.00 L tank at 22.7 °C is filled with 6.21 g of sulfur hexafluoride gas and 7.82 g of boron…

A:

Q: A 5.00 L tank at 12. °C is filled with 14.2 g of chlorine pentafluoride gas and 3.58 g of sulfur…

A:

Q: Calculate the mass and number of moles of dinitrogen difluoride gas that were collected. R

A: Given: Volume= 30.0 L Pressure= 0.320 atm Temperature= 8.0oC= 281.15 K   To calculate:

Q: A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 g of dinitrogen…

A:

Q: ired to decrease the volume of the gas sample to 7.44 L, p 0.540 atm, the temperature of the gas…

A: Initial Volume = 9.40 L Initial Temperature =53 °c = 326 K Initial pressure = 0.440 atm Final…

Q: When heated, mercury (II) oxide (HgO) decomposes to give O2 gas. 2 HgO (s) → 2 Hg (l) + O2 (g) What…

A: From the above reaction we can see that 2 moles of HgO is decomposing to form 1 mole of O2  hence…

Q: A gas mixture in a 4.600 L container at 350°C contains 1.35 g each of Ar, CO, and CH4. Find the…

A: The term number of moles has been defined as the ratio of mass to the molar mass of the given…

Q: A 9.00 L tank at 1.9 °C is filled with 15.6 g of dinitrogen difluoride gas and 11.7 g of sulfur…

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Q: A gas exerts a pressure of 1atm at standard temperature. What should be the new temperature (in…

A:

Q: A mixture of CH4 (g) and C₂H6 (g) has a total pressure of 0.54 atm. Just enough O2 (g) is added to…

A: Solutions         Hence the mole fraction of methane 0.6018

Q: A large flask with a volume of 936 mL is evacuated and found to have a mass of 134.66 g. It is then…

A:

Q: The gas of a certain volcano had the following composition in mole percent: 60.0% CO2, 28.0% H2,…

A: To calculate partial pressure of CO2:

Q: A gas mixture contains 2.5 mol N2 and 9.7 mol CO2, and has a pressure of 2.3 atm. What is the…

A: No of moles of N2 = 2.5 mol. No of moles of CO2 = 9.7 mol. Total pressure = 2.3 atm.

Q: A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the…

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: use the ideal gas law to identify this gas.

A: Ideal Gas Law :-  PV = nRT  P is the pressure of gas  V is the volume occupied by gas n is the…

Q: Dinitrogen difluoride gas is collected at 10.0 °C in an evacuated flask with a measured volume of…

A:

Q: moles

A:

Q: A 6.00 L tank at 6.04 °C is filled with 18.4 g of sulfur hexafluoride gas and 2.89 g of carbon…

A: Given that:  Mass of sulfur hexafluoride (SF6) = 18.4 g Mass of carbon dioxide (CO2) = 2.89 g…

Q: A 10.0 L tank at 8. °C is filled with 17.7 g of sulfur hexafluoride gas and 5.37 g of boron…

A: Given: Volume of tank = 10.0 L Temperature = 8 oC Mass of sulfur hexafluoride i.e. SF6 = 17.7 g. And…

Q: Calculate the partial pressure of helium gas for a volume of 1.0 x 10-6 m3 of 222Rn gas after 9…

A:

Q: A sample of a smokestack emission was collected into a 1.10-L tank at 742 mm Hg and analyzed. The…

A: In 100 g sample mass of CO2= 92 g  Mass of NO = 4.2 g  Mass of SO2 =1.3g Mass of H2O = 2.5g  Molar…

Q: To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an…

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Q: The ideal gas law describes the relationship between pressure (P), temperature (T), volume (V), and…

A: For ideal gas , variables pressure , temperature and volume are related as shown by ideal gas…

Q: A 5.0 × 102 sample of sulfur dioxide, SO2(g), has a volume of 2.37 × 106 L. If the temperature of…

A:

Q: The label on a cylinder of a noble gas became illegible, so a student allowed some of the gas to…

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Q: A 8.00 L tank at 2.97 °C is filled with 17.8 g of sulfur tetrafluoride gas and 4.54 g of carbon…

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Q: Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of…

A: The question is based on the concept of gaseous state. we have to calculate total pressure of the…

Q: A student obtained a mass of 0.266 g CO2 during his experiment. The atmospheric pressure was 751.6…

A:

Q: A 8.00 L tank at 29.8 °C is filled with 14.1 g of chlorine pentafluoride gas and 17.2 g of boron…

A:

Q: A 8.00 L tank at 11.8 °C is filled with 7.85 g of carbon dioxide gas and 3.51 g of boron trifluoride…

A: Volume = 8.00 Lmass of CO2 = 7.85 gmolar mass of CO2 = 44.01 g/molmass of BF3 = 3.51 gmolar mass of…

Q: A 9.00 L tank at 8.6 °C is filled with 11.0 g of sulfur tetrafluoride gas and 9.86 g of dinitrogen…

A: Answer: Mole fraction of a gas in a gaseous mixture is always equal to the ratio of the moles of the…

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.