You will need the following data:R = 8.314 kPa L molK1I from the information above in KelvinV from the information above in LP in kPaNote: the units all have to be in the same form when used in calculations!!!100% H2O2 density is 1.45 g/mL5 mL of a solution containing an unknown concentration of hydrogen peroxide wasdecomposed at 25 °C releasing 48 mL of gas. The temperature of the container used to measure the volume of gas produced was 20 °C.To find BOTH the concentration of hydrogen peroxide in the solution AND the percentage of hydrogen peroxide in solution work through the following steps.1.Rearrange the ideal gas law to solve for n.2. Convert the temperature of the water in the collection vessel from °C to Kelvin (K). Therefore: T =3.Convert the current barometric pressure in the room from hPa to kPa. The Macquarie university weather station data can be used to find the pressure http://aws.mq.edu.au.Use the current pressure which is given in hectopascals. Use 1018 hPa if unavailable.10 hPa = 1 kPa So divide hPa by 10 to convert to kPa.Convert the volume of oxygen from mL to Liters and solve for the number of moles ofO2. Be sure the units cancel so that you end up with only the moles of O2.

2.51 A tank contains 20 L of compressed nitrogen at 10 bar and 25 °C. Calculate the maximum work that can be obtained when the gas is allowed to expand reversibly to 1 bar pressure(a) isothermally and (b) adiabatically. The heat capacity of nitrogen at constant volume can be taken to be 20.8 J K mol^-1 independent of temperature.

Problem 3.33 Within a cubic unit cell, sketch the following directions: Required problems are a, d, and g. The remaining problems are optional but are provided for addedpractice. Solutions will be provided for all of these problems.

ESCIb) The following temperature/composition data were obtained for a mixture of two liquids A and B at 1,00 atm, where x is the mole fraction in the liquid and y the mole fraction in the vapour at equilibrium.

1.14 The isothermal compressibility K of a gas is defined in Problem 1.17, and its value for an ideal gas is shown to be 1/P.Use implicit differentiation of V with respect to P at constant T to obtain the expression for the isothermal compressibility of a van der Waals gas. Show that in the limit of infinite volume, the value for an ideal gas is obtained.

ESC.1la) The following temperature-composition data were obtained for a mixture of octane (O) and methylbenzene (M) at 1.00 atm, where x is the mole fraction in the liquid and y the mole fraction in the vapour at equilibrium. The boiling points are 110.6°C and 125.6 °C for M and O, respectively. Plot the temperature-composition diagram for the mixture. What is the composition of the vapour in equilibrium with the liquid of composition (i) x,, = 0.250 and(ii) x, = 0.250?

ESAI(a) A water carbonating plant is available for use in the home and operates by providing carbon dioxide at 5.0 atm. Estimate the molar concentration of CO, in the carbonated water it produces.

4-66 5 kg of Argon is compressed in a polytropic process with n = 1.2 from 120 kPa and 108"C to 800 kPa in a piston-cylinder device. Determine the work produced and heat transferred during this compression process.

1.6 Show how the second virial coefficient of a gas and its molar mass can be obtained by plotting P/p versus P, where p is the density of the gas. Apply this method to the following data on ethane at 300 K. P/bar 1 10 20 p/10^-3 g cm^-3 1.2145 13.006 28.235

9.46 An atom makes a transition from an excited state with a lifetime of 10-9 s to the ground state and emits a photon with a wavelength 600 nm. What is the uncertainty in the energy of the excited state? What is the percentage uncertainty if the energy is measured from the ground state?

Which stresses will cause the concentration of chlorine gas toincrease? \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})<\mathrm{PCl}_{5} \text { i) increasing the temperature } ii) increasing the concentration of PCI3 iii) decreasing the pressure Question 7 options: a. i, ii, and iii b. i and ii only c. i and iii only d. ii and iii only