Calculate pressure in atm exerted by 3 mol of CO2 behaving as a van der Waals gas in a 22.414 L vessel at 273.15 K. Van der Waals parameters for CO2 are a = 3.61 atm L^2mol^-2 and b= 4.49 (1)^-2 L/mol

Q: A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the…

A: Given: Volume of the cylinder=1.00L Number of moles= 1 mol Temperature= 25°C=298K

Q: The atmosphere of a planet is mostly carbon dioxide gas. At the surface of the planet, the…

A: The STP condition on the planet that mostly contains carbon dioxide gas are as follows: Temperature…

Q: According to the ideal gas law, a 9.045 mol sample of oxygen gas in a 0.8496 L container at 499.8 K…

A: The pressure of O2 gas under the given conditions has been calculated using ideal and Vanderwaal's…

Q: 313 K according to the reaction below. During the reaction, the pressure and temperature change. In…

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

Q: Use both the Ideal Gas Law and the van der Waals equation to calculate the pressure exerted by a…

A: Solution ) The pressure of the gas can be calculated by ideal gas equation as well as vander waal…

Q: According to the ideal gas law, a 0.9926 mol sample of nitrogen gas in a 1.567 L container at 266.4…

A: The expresssion for ideal gas equation is shown below: PV = nRT where,  P = pressure of ideal gas V…

Q: An 89.3 mL sample of wet O2(g) is collected over water at 21.3°C at a barometric pressure of 756…

A: Given :-  Volume of wet oxygen =  VwO2 = 89.3 mL  Total Pressure = Ptotal = PdO2 = 756 mmHg  Vapor…

Q: A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the…

A:

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A:

Q: 10. (a) Calculate the amount of gas present in a 500 mL container at 27°C and 1.7 atm of pressure.…

A:

Q: Calculate the molecular mass of a liquid that, when vaporized at 100 °C and 755 Torr, yields 185 mL…

A: Gas equation, PV = nRT

Q: According to the ideal gas law, a 10.17 mol sample of xenon gas in a 0.8242 L container at 499.1 K…

A: The objective of the question is to calculate the percent difference.

Q: A 1.90 g sample of elemental lithium,Li(s) is reacted with water, yielding lithium hydroxide, LIOH,…

A: The balanced reaction given is, => Given: Mass of Li reacting = 1.90 g. Temperature at which the…

Q: Calcium carbide reacts with water to produce acetylene gas according to the following equation…

A: The given reaction is shown below.

Q: Neon effuses at a rate of 0.325 moles per second at certain volume, pressure, and temperature. How…

A:

Q: In an attempt to determine an accurate value of the gas constant, R (L atm K-1 mol-1), a student…

A:

Q: A mixture of xenon and methane gases contains xenon at a partial pressure of 354 mm Hg and methane…

A: Partial pressures of xenon and methane are given. We have to calculate the mole fractions of Xe and…

Q: A 1.00 L rigid cylinder contains one mole of neon gas at 25 °C. Calculate the pressure using (a) the…

A: Given,Volume (V) = 1.00 LNumber of moles (n) = 1 molTemperature (T) = 25 oC = 298 K

Q: Using (a) the ideal gas law and (b) the van der Waals equation, calculate the pressure exerted by…

A: Ideal gas equation PV=nRTP=pressure of the gasV=volume of gasn=number of molesR=gas…

Q: Calculate the pressure that CC14 will exert at 80 °C if 1.00 mol occupies 33.3 L, assuming that (a)…

A: Ideal gas equation: PV=NRT Van der Waals equation: P=nRTV-nb-an2V2 where a and b are van der Waals…

Q: A piece of dry ice (solid carbon dioxide) with a mass of 5.49 gg is placed in a 10.0-LL vessel that…

A: Well, we will first convert the mass of Carbon dioxide to moles. And using the ideal gas equation,…

Q: According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K…

A: To calculate the percent difference between the pressure predicted by the ideal gas law and 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.