How to obtain the relative mean

Q: To derive the Maxwell relation, write the equation giving the total change of energy starting with…

A: In this question we have to derive the given Maxwell equation.

Q: What is the kinetic energy of an ideal gas at absolute zero?

A: Kinetic energy of an ideal gas is given by the expression KE=32KT

Q: What is the mole fraction

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Q: Silicon tetrachloride(SiCl4)and trichlorohydrosilicon(SiHCl3) are both starting material of…

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Q: If n and V are constant, q is equal to

A: Given : n and V are constant.

Q: Use the following picture to solve for a and b.

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Q: mean mass and the average deviation from the mean.

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Q: Justify the formulation of the van der Waals equation of state.

A: There are two types of gases are studied in gaseous phase. One is ideal and other is real gas. A gas…

Q: Explain with the diagram the experimental method to find the equation for an ideal gas

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Q: What is the value of standard temperature and pressure?

A: What is the value of standard temperature and pressure?

Q: Use the Vanderwalls equation and the ideal gas equation to calculate the volume of 2 Mol of Ar at a…

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

Q: Which statement A-D regarding an ideal gas is not correct?

A: According to ideal gas equation    PV= nRT  where P is pressure, V is volume, n is number of moles,R…

Q: Compute for the partial pressure of each gas in the mixture.

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Q: mole fraction for th

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Q: Write out the equation for the First Law in differential form and define each term.

A: The first law of thermodynamics can be described as the change in internal energy is equal to the…

Q: Calculate the max using Woodward-Fieser Rules

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Q: If PV = nRT, then solve for T.

A: A question based on general chemistry that is to be accomplished.

Q: For a pure substance, I. Mass II. Inertial property III. Density Which ones of the above properties…

A: There are intensive and extensive properties of substance . The intensive properties are independent…

Q: How would I turn the first equation to fit into the second one? I can’t figure out how to get or…

A: First equation represent relative error. Difference of actual and experimental value is absolute…

Q: How to assume if the gas mixture behave ideally?

A: There are following assumptions to assume a gas is behaving ideally:

Q: a. Do the given data follow's Charles' Law? b, Generate the equation of the line that best fit the…

A: We need to check the plot between T and V.

Q: Find the relation of the constants a and b of the Berthelot equation to the critical constants.

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Q: s volume if th

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Q: Write an expression for the new temperature of the sample, and (possibly using numerical…

A: The new temperature of the sample can be calculated as follows:

Q: variation of the total pressur 1 (P¡ = 1008 Torr) and n-de nction of the mole fraction

A: Given as, isopropanol= 1008 Torr, n-decane= 48.3 Torr.

Q: Explain the significance of the constants a and b in the van der Waals equation of state.

A: We have to explain the significance of constants a and b in the Vander Waals equation of state.

Q: A mole of ideal gas has a specific volume at a given temperature independent of identity of the gas…

A: For calculation of molar volume at 310 K we have to use the following equation:…

Q: e partial pressures of

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Q: A vessel at 500 K contains O, and N, with number densities of 1023 m-3 and 1024 m-3. What is the…

A: Given: The number density of O2 = 1023 m-3 And the number density of N2 = 1024 m-3

Q: Show that at a critical point, the first and second derivatives of the pressure with respect to the…

A: Consider the given gas behave as real gas and its first derivative for the isothermal process is…

Q: What is the difference between a false positive and a false negative?

A: Given terms,         False positive and a false negative

Q: mole fraction of the methanol?

A: Given data are as follows: Methanol weight= 40 g Ethanol molecular weight= 60 g

Q: At constant pressure, the volume of a fxed mass of an ideal gas is directly proportional to the…

A: It states that, for a given mass of an ideal gas at constant pressure, the volume is directly…

Q: For the function: R, a, b - are constant - Write an expression for the derivative of p in relation…

A: Equation of gas given:                                                                         P=…

Q: The atmospheric surface pressure on Venus is 90 bar and is composed of 96% carbon dioxide and…

A: Given:- Pressure of Venus surface (P) = 90 bar Composition of CO2= 96% Composition of other gases =…

Q: at volume

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: approaches infinity in the virial equation of state, a real As the gas will start to behave as an…

A: Please find your solution below : Virial equation of state is an equation that describes the…

Q: 300 0ml of a00s at 100atm and 27°C would require what temperature to change to 1.00L and

A: As per instructions we are allowed to answer  one question , so i answered second question

Q: Write the expression to solve for x in a quadratic equation.

A: Answer :-               x = - b ± b2 - 4ac2a

Q: alid between 298-700 K, 0.012643 (T)=18.42+ 24.647 – 8.9147² +9.6657³ J mol K

A: Solution -

Q: expression that relates total pressure of gas to the total kinetic energy of an Derive an ensemble…

A: The pressure of a gas is equal to the total kinetic energy of the molecules in a unit volume of the…

Q: Using partial derivative determine the change of pressure with respect to volume, all else constant…

A: Ideal gas law gives the behavior of ideal gases and how its temperature, pressure, volume and no. of…

Q: units of k?

A: Unit of k is : L.mol-1.s-1

Q: diffrentiate between the physical and chemical effects of pressure

A: The physical and chemical effects of pressure can be explained by considering an gaseous equilibrium…

Q: determined by two variables, which are as follows?

A: Partial pressure is the pressure exerted by a particular gas in the gaseous mixture.  Partial…