Find the temperature in ˚ C of 0.792 moles of hydrogen gas with a volume of 18639 mL collected at a 761.88 torr. The gas was not collected over water. The ideal gas constant, R = 82.1 atm·mL/mol·K. The ideal gas equation is: PV=nRT

Q: A mixture of cyclopropane gas, C3H6, and oxygen, O2, in a 1.00:4.00 mole ratio is used as an…

A: Answer :- 84800 Pa  The partial pressure of O2 = 84800 Pa.…

Q: The temp of an ideal gas in a 5 . 00 L container originally at 1 . 0 atm pressure and 2 5 C is…

A:

Q: Consider the sample 7.85 moles of CO2 gas at 37°C and 1.2 atm. (a) Find the mass of 7.85 moles of…

A: The objective of the question is to calculate the mass, volume and density of 7.85 moles of CO2 gas…

Q: Calculating partial pressure in a gas mixture A 8.00 L tank at 25.3 °C is filled with 4.35 g of…

A: Calculation  of mole fraction  of CO2 and N2F2 and partial pressure  and total pressure  of flask.

Q: To identify a diatomic gas (X2X2), a researcher carried out the following experiment: She weighed an…

A:

Q: determine the temperature

A:

Q: A cylinder of volume 27.0 L is filled with 25.1 g of jobstium gas (MM = 72.21 g - mol-1) from the…

A: Given data, Mass = 25.1 g Molar mass = 72.21 g/mol.  To calculate the number of moles.

Q: A 5.00 L tank at 29.6 °C is filled with 17.3 g of boron trifluoride gas and 12.8 g of chlorine…

A:

Q: Calculate the following quantities for an ideal gas: The absolute temperature of the gas at which…

A: Given, Number of moles of gas = 3.75 x 10-3 moles Temperature = ? Pressure of gas = 0.945 atm Volume…

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 gas with a mass of 95.14g occupies 48.8L at 659mmHg and 25.3°C. What is its molecular weight? Use…

A:

Q: Calculate the volume of ammonia gas, measured at STP for the complete reaction of 25 g of quicklime…

A: According to Gas law, PV = nRTNow at STP, Pressure =1 atmT = 273 KR = 0.0821 LatmmolK   From this…

Q: Consider the reaction of 1.41 g Ca(s) with 107 mL of 0.325 M HBr(aq) according to the following…

A: The reaction taking place is given as, => Ca (s) + HBr (aq) -----> CaBr2 (aq) + H2 (g) Given :…

Q: lorine is widely used to purify municipal water oplies and to treat swimming pool water. ppose that…

A: Given that: V1 = 8.60L P1 = 890 torr T1 = 25°C = 25°C+273 = 298K V2 = 6.90L T2 = 56°C = 56°C+273 =…

Q: Suppose 10.05 mol of Ar gas are pumped into a 1.01 L container at 293.15 K. part 1:Calculate the…

A: Here we are required to find the pressure of Argon gas both ideally and non ideal scenario

Q: An unknown gas has a density of 1.48 g/L and a molar mass of 68.2 g/mol. You have measured the…

A: For the ideal gas, the temperature pressure and the volume are related by the ideal gas equation.…

Q: Consider a gas mixture that contains only helium (He) and neon (Ne). If the partial pressure of He…

A:

Q: A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 g of chlorine…

A:

Q: A 9.00 L tank at 5.93 °C is filled with 7.54 g of boron trifluoride gas and 17.1 g of dinitrogen…

A: Partial pressure = total pressure x mole fractions of the gas. Using this formula , calculate the…

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

A: Using the ideal gas equation, we can calculate the molar mass of the diatomic gas.The ideal gas…

Q: A flask contains 740 mmHg of nitrogen (N2) gas in a 4.00 L container at 25.0 °C. If 44.0 g of carbon…

A:

Q: A sample of an unknown compound is vaporized at 100. °C. The gas produced has a volume of 1840. mL…

A: Answer:Here:

Q: A student recovered0.398g of THF vapor in a 125 mL flask. Assuming the vapor is an ideal gas with a…

A:

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: To identify a diatomic gas (X2X2), a researcher carried out the following experiment: She weighed an…

A: Using the ideal gas equation, we can calculate the molar mass of the diatomic gas.

Q: A 9.00 L tank at 8.36 °C is filled with 4.08 g of sulfur hexafluoride gas and 10.8 g of boron…

A:

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: of 93.65g occupies 47.8L at 734mmHg and 32.7°C. What is A gas with a mass its molecular weight?

A: The combination of Boyle's law, Charles's law and Avogadro's law leads to an equation which shows…

Q: Calculating partial pressure in a gas mixture A 8.00 L tank at 9.28 °C is filled with 6.17 g of…

A: The objective of this question is to calculate the mole fraction, partial pressure of each gas, and…

Q: 215.0 mol of an unknown gas is stored at a temperature of 1110 K in a large, 395 L container. In…

A: Pressure is calculated by using ideal gas equation

Q: Use the ideal gas equation, PV = nRT, to calculate the volume in liters of 1.808 moles of nitrogen…

A: The ideal gas law was directly used to find the volume.

Q: A 10.00 L tank at -7.6 °C is filled with 5.09 g of chlorine pentafluoride gas and 16.3 g of…

A:

Q: A 5.00 L tank at 8.18 °C is filled with 17.3 g of sulfur tetrafluoride gas and 4.95 g of chlorine…

A:

Q: A 10.0 L tank at 22.3 °C is filled with 7.78 g of carbon dioxide gas and 9.60 g of dinitrogen…

A: The temperature of the gas sample is = 22.3oC = 22.3+273.15 = 295.45 K The volume of the tank is =…

Q: An ideal gas is contained in a cylinder with a volume of 5.1*10^2 mL at a temperature of 30.°C and a…

A: An ideal gas has negligible volume in compare to volume of the container, and the molecules of ideal…

Q: What is the pressure in a 19.0 L cylinder filled with 0.681 mol of nitrogen gas at 322 K? VO AE ΑΣφ…

A:

Q: A 7.00 L tank at 6.54 °C is filled with 17.3 g of sulfur tetrafluoride gas and 17.7 g of chlorine…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 17.3 g Mass of chlorine pentafluoride i.e ClF5 = 17.7…

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.