Calculate the temperature of each of the following systems. Show your working. (i) 6 x 1022 molecules of helium gas occupying 2.0 litres at atmospheric pressure.
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Calculate the temperature of each of the following systems. Show your working.
(i) 6 x 1022 molecules of helium gas occupying 2.0 litres at atmospheric pressure.
(ii) A system of particles occupying non-degenerate energy levels with the following population distribution:
Energy (J)
4.823 x 10-21
3.445 x 10-21
Population
3.1%
8.5%
2.067 x 10-21
23 %
6.889 x 10-22
63%
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- Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.Let temperature in 3-space be given by T(x, y, z) = x2 - y2 - z.Draw isotherms corresponding to temperatures T = -1, 0, 1.21.7 g of a basic solution was mixed with 87.6 g of water in a calorimeter with a calorimeter constant of 47.6 J K–1 with all substances initially at 29.3 °C.The resulting solution was observed to be at a temperature of 15.4 °C and have a heat capacity of 4.39 J g–1 K–1.Determine q for the mixing process. a. 6670 J b. -1.37 × 105 J c. -7330 J d. -6670 J e. 7330 J
- a) A 1.60 dm3 sample of a mixture of methane gas, CH4 and oxygen gas, measured at 25 oC and 101 kPa, was allowed to react in a bomb calorimeter in which, had a heat capacity of 5.30 kJ/K altogether with its contents. The complete combustion of the methane gas to carbon dioxide gas and water caused a temperature rise in the calorimeter of 6.28 K. Given that ∆Ho c (CH4) is -560 kJ/mol. i. Define the standard enthalpy of combustion of methane ii. Write a thermochemical equation for the combustion of methane iii. Knowing the ∆Ho c of methane, calculate the number of mole of methane in the mixture. iv. Calculate the total moles of gases in the calorimeter.Calculate the work of expansion accompanying the complete combustion of 10.0 g of sucrose (C12H22O11) to carbon dioxide and (a) liquid water, (b) water vapour at 20 °c when the external pressure is 1.20 atm.A piston/cylinder setup contains 1 kg of air at 20°C with an initial volume of V1=0.1 m3, as shown in Fig. Q7. Initially, the piston rests on some stops, but it is possible for it to move within the cylinder without friction. To lift the piston and start such motion, an air pressure of 1400 kPa is required. Now, heat is transferred to the system so that the temperature of the air reaches to a final value of 300°C. Fig. Q7 A. Which statement is true? The air can lift the piston before the temperature reaches to 300°C The air cannot lift the piston before the temperature reaches to 300°C
- a chemist carefully measure the amount of heat needed to raise the temperature of a 0.60 kg sample of a pure substance from 47.3 c tp 53.3c. the experiment shows that 15. kj of heat are needed. what can the chemist report for the specific heat capacity of the substance? round to 2 sig figs.. A 2.50 mole sample of a perfect gas for which Cv,m = 3R/2 (assume constant over T-range) undergoes the following two-step process: (1) from an initial state of the gas described by T = 13 ºC and P = 1.75 x 105 Pa, the gas undergoes an isothermal expansion against a constant pressure of 3.75 x 104 Pa until the volume has doubled. (2) subsequently, the gas is cooled at constant volume. The temperature falls to -24ºC. Calculate q, w, ∆U, and ∆H for each step and for the overall process.Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively Calculate the work done when 1.0 mole of nitroglycerin decomposes and additionally explain the significance of the sign.
- The heat capacity (Cp) 0f an hal0genated 0rganic c0p0und, chl0r0f0rm is given by the f0ll0w equati0n. Equati0n (1) Cp (J/mol K) = 19.8 +0.22 T – 0.00026 T2 (a) 0btain a new equati0n that uses T in Fahrenheit (b) Calculate the Cp 0f chl0r0f0rm at 300 K using Equation (1) (c) Calculate the Cp 0f chl0r0f0rm at 80 F using the equati0n you derived in (a)The growth of the bacterium Zymomonas mobilis in ethanol under aerobic conditions is described by the following global reaction:C2H5OH + a O2 + b NH3 → c C H1.704N0.149O0.408 + d CO2 + e H2Oa) Write the equations for the balance by elements and the balance of electrons.b) determine the coefficients a, b, c, and d knowing that RQ = 0.66c) determine YX/S and YX/O2A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0125 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.4ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.