A sample of gas at 2455 torr is cooled from 150.0 °C to 100.0 °C. Assuming the volume is constant, what is the pressure (in atm) of the gas at 100.0 °C?

Q: A sample of argon gas at a pressure of 0.752 atm and a temperature of 25.8 °C, occupies a volume of…

A: Given data, Initial pressure (P1) = 0.752 atm Initial volume (V1) = 441 mL Final Pressure (P2) =…

Q: At constant temperature, the pressure on a 6.0 L sample of gas is increased from 1.0 to 2.0 atm.…

A: Boyle's law This law states that the absolute pressure exerted by a given mass of an ideal gas is…

Q: A 16.3 L sample of neon at 25.0°C and a pressure of 745 torr is kept at 25.0°C as it is allowed to…

A: Given :-  Initial pressure =745 torr Initial volume = 16.3 L Final volume = 21.2 L  Temperature =…

Q: Calculate the final pressure of a gas in atm that was initially occupying 47.44 cm³ at 670.93 mmHg…

A: We have to calculate the final pressure.

Q: Convert 747.6 mmhg to atm

A: 1 atm = 760 mm Hg  Thos conversion factor will be used to convert mm Hg to atm

Q: mol sample of hydrogen gas at a temperature of 12.0 ers. The pressure of this gas sample is mm

A: Given, Mole(n) = 0.906 mol Temperature (T) = 12.0 °c = 285 K Volume (V) = 23.6 L Gas constant (R)=…

Q: tank contains helium gas at 473 mmHg, nitrogen gas at 0.719 atm, and neon at 572 torr.  Calculate…

A: Total pressure is equal to sum of pressure of all gases

Q: If 48.070 L of gas is collected at a temperature of 20.531°C and a total pressure of 798.00 torr,…

A: The given data contains, Volume = 48.070 L. Total pressure = 798 torr. Temperature = 293.531 K

Q: The volume of a gas decreased to from 1.00 L to 600. mL while the temperature remain constant. If…

A: Answer - According to the question - Given values are - Pressure = 720 Torr Volume of gas =  1.00 L…

Q: 0.638 mol sample of xenon gas at a temperature of 25.0 °C is found to occupy a volume of 22.6…

A: number of moles = 0.638 mol Volume = 22.6 L Temperature = 25.0 °C = 298 K Gas constant , R =…

Q: A sample of nitrogen gas occupies a volume of 8.57 L at 69.0°C and 365 torr. If the volume of the…

A: Given  Initial Pressure (P1)  =365 torr Initial Temperature (T1)  = 69 ℃…

Q: At constant temperature the pressure on a 6.0 L sample of a gas is reduced from 1.00 atm to 1140…

A: Formula used: PV=nRT Given data: P1=1atm = 760torr P2=1140torr V1=6L

Q: Calculate the partial pressure of a hydrogen gas sample collected over water at 30 degree C if the…

A:

Q: A fixed amount of gas at 25.0 °C occupies a volume of 8.66 L when the pressure is 629 torr.…

A:

Q: A fixed amount of gas is in a rigid container at room temperature (25.0C). If the gas pressure…

A: Given that: Initial temperature (T1) = 25.0°C Initial pressure (P1) = 1.50 atm Final pressure (P2) =…

Q: Determine the density of F2 gas at 273 K, 1.00 atm. The molar mass of F2 is 38.0 g/mol.

A: We will use ideal gas equation

Q: 0.743 mol sample of nitrogen gas at a temperature of 23.0 °C is found to occupy a volume of 20.7…

A: Since PV = nRT  where P = pressure in atm  V = volume in L = 20.7 L n = moles = 0.743 T =…

Q: A sample of hydrogen gas at a pressure of 940 mmHg and a temperature of 79°C, occupies a volume of…

A: According to ideal gas law, PV = nRT where P = pressure V = volume n = moles R = gas constant T =…

Q: The initial volume of a nitrogen gas is 2.5 L. What is the final volume of the nitrogen gas (the…

A: Given: Initial volume = 2.5 L Initial pressure= P  Final pressure= P/3 Initial temperature= T Final…

Q: 0.862 mol sample of helium gas at a temperature of 6.00 °C is found to occupy a volume of 27.7…

A: Answer:Here:

Q: When 4.67 L of carbon dioxide at 485.6 mmHg and 25.0 ℃ is heated to 475.0 ℃ and converted to 754.2…

A: Given P1 = 485.6 mmHg V1 = 4.67 L T1 = 25°C P2 = 754.2 mmHg V2 = ? T2 = 475°C

Q: The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant…

A: According to Boyle's law, the variation of pressure and volume of an ideal gas at constant…

Q: Convert 562.7 mm Hg into atmospheres.

A: Unit conversion is an important concept to convert the given units into others by using the…

Q: Three gases are present inside an 20.0L chamber. Argon is present at a partial pressure of 154 torr,…

A: Given that a 20.0L chamber contains,  Partial pressure of Argon gas pAr   = 154 torr Partial…

Q: A sample of xenon gas at a pressure of 0.806 atm and a temperature of 27.7 °C, occupies a volume of…

A:

Q: If a gas with a volume of 10mL and a pressure of 236 torrs inside a dewar flask is opened to an…

A:

Q: A mixture of xenon and nitrogen gases is maintained in a 5.74 L flask at a temperature of 67°C. If…

A: Dalton's law of partial pressures states that in a mixture of non-reacting gases, the total pressure…

Q: sample of xenon gas at a pressure of 0.577 atm and a temperature of 23.9 °C, occupies a volume of…

A: At constant Temperature,  Using Boyle's law,  P1V1 = P2V2  0.577 × 12.6 = P2 × 19.4 P2 = 0.375 atm

Q: A sample of gas at 2085 torr is cooled from 150.0 °C to 100.0 °C. Assuming the volume is constant,…

A:

Q: 0.9110 grams of an unknown gas was placed into an evacuated 0.500 L container. The temperature was…

A: The ideal gas equation is  PV = nRT  PV = (m/M)RT P = pressure  V = volume  n = moles of gas = mass…

Q: The volume of a 1.00 g sample of Ne gas at 30.0 °C is 250 mL. What is the pressure (in atm) of the…

A: According to ideal gas, the product of pressure and volume is equal to the product of no of moles,…

Q: A sample of gas has a pressure of 756 mmHg in a 125-mL flask. The sample of gas is transferred to a…

A: Boyle’s Law Example Problem

Q: The pressure on a sample of an ideal gas is increased from 0.941 atm to 3.55 atm at constant…

A: Here given--- Initial Pressure (P1) = 0.941 atm Initial volume (V1) = 482 mL = 0.482 L Final…

Q: If a balloon is filled with 4.56 moles of helium gas and then exposed to a pressure of 0.123 atm at…

A: Given: Moles of He  gas: 4.56 Pressure : 0.123 atm Temperature : 28 oC = 301 K

Q: A sample of neon gas occupies a volume of 8.94 L at 55.0°C and 333 torr. If the volume of the gas…

A: From the ideal gas law equation, PV = nRT; where P is for pressure, V is for volume, n is the number…

Q: A sample of xenon gas occupies a volume of 7.28 L at 65.0°C and 367 torr. If the volume of the gas…

A:

Q: A sample of hydrogen gas occupies a volume of 8.56 L at 68.0°C and 313 torr. If the volume of the…

A: Given, Initial volume(V1) = 8.56L Initial temperature (T1) = 68°C = 273 + 68= 341K Initial pressure…

Q: A sealed sample of fluorine gas has a pressure of 6.80 atm at a temperature of 9.0°C. If the volume…

A:

Q: sample of argon gas is held in a sealed container at a pressure of 2.24 atm at 48.0°C. What will the…

A: At constant volume and mole , pressure of gas is directly proportional to temperatures

Q: What was the final pressure (in torr)

A:

Q: A sample of gas at 43.67 K exerts a pressure of 1.56 atm. Calculate the final pressure if the…

A: Gay-Lussac's gives the relation between pressure and the temperature of the gas. Pressure is…

Q: A sample of 10.2 liters of an ideal gas at 23.0 °C and 750.5 torr is compressed and heated so that…

A: According to the ideal law of pressure, the volume of a gas is directly proportional to the number…

Q: partial pressure

A:

Q: A fixed amount of gas at 25.0 °C occupies a volume of 8.66 L when the pressure is 629 torr.…

A: The solution is given below -

Q: 0.746 mol sample of carbon dioxide gas at a temperature of 12.0 °C is found to occupy a volume of…

A: Given data :  Moles of carbon dioxide , n = 0.746 mol  Temperature,  T = 12.0°C  Volume,  V = 22.0…

Q: sample of nitrogen gas initially occupies a volume of 27.5 L at a temperature of 22.5 °C and a…

A:

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.