Post-lab Calculations: 1. Calculate the specific heat, for both trials, by setting heat gained by the water (qw) to heat lost by the metal (qm). Trial 1: Trial 2:
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- Q1) A constant volume tank contain 1 mole ofC7H14and 12 mole of O2 gas at a temperature of 25 °C and 1 bar. The contents of the tank is ignited and C7H14 is burned completely and final products temperature is found to be 1700 K. Determine the heat transfer during this process. ( take daltaHo = -47800 kJ/kg).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°CConsider one mole of an ideal monoatomic gas at STP and confined in a volume V1. You would like to increase its temperature by an amount ΔT.a) Where will you provide less heat to achieve your objective; at constant volume process or at constant pressure process? Give your reasoning without using or referring to any formula.b) We can achieve the same objective along an adiabatic process; how do we do it keeping in mind that there is no heat exchanged in an adiabatic process?c) Express the work done by the gas in the three processes; the question is not merely to write the expressions but you must show briefly how they are obtained.
- One mole sample of an ideal, monoatomic as initially has a molar volume of 24.45 liters per mole at 1 bar and 298.2 Kelvins, It was expanded adiabatically and reversibly to 187.8 Kelvins where the molar volume increased to 48.90 liters per mole. How many KiloJoules of work is involved in the process. Express answer in three sig figs.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.Determine the theoretical flame temperature that can beobtained by the combustion of methane with 25% excess air.Air and methane enter at 298K and a pressure of 1 atm. Thereaction is complete. Standard heat of formation at 298 inkJ/kmol are: Methane (g) = -74520, CO2 (g) = -393500, Watervapor (g) = - 241813.
- To properly determine the internal energy of combustion methylhydrazine, the calorimeter was first calibrated. A 0.4500 g sample of sucrose (MW 342.296 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.98 K. For sucrose, the internal energy combustion at constant volume, ∆U, is known to be –5616.64 kJ/mol. Calculate the calorimeter constant, in kJ/K.Oxygen at 150 K and 41.64 atm has a tabulated specific volume of 4.684 cm3/g and a specific internal energy of 1706 J/mol.(a) The figure 1706 J/mol is not the true internal energy of one g-mole of oxygen gas at 150 K and 41.64 atm. Why not? In a sentence, state the correct physical significance of that figure. (The term “reference state” should appear in your statement.)(b) Calculate the specific enthalpy of O2 (J/mol) at 150 K and 41.64 atm, and state the physical significance of this figure. What can you say about the reference state used to calculate it?Ethane in a closed system is compressed without friction from 95 to 190 kPa in such a manner that pV=constant. Initially, the density is 1.11 kg/m3 and the volume is 0.045 m3. During the compression, 2.96 kJ of heat is removed from the ethane. Determine the change in internal energy of the ethane.
- Calculate Q (system) (J) and delta H (kJ/mol). Use data below and from methods: Mass of NaNO3 required (already calculated) = 8.5 grams Initial Temperature ti (0C) = 25.0 0C Temperature after 240 sectons (tf, final temp) = 19.0 0C Measuring the heat evolved or absorbed methods Weigh the calculated mass of NaNO3 needed to prepare 100mL of a 1.0M solution. Place 100mL of distilled water in the calorimeter and carefully add the solid NaNO3. Begin stirring and measure the temperature of the solution to the nearest 0.10C after 30seconds and every 30 seconds thereafter until the temperature attains either a maximum or minimum which is the final temperature tf. Calculate q(system), using specific heat=4.184J/g.0C, density ofsolution=1.0g/mL; heat capacity of calorimeter = 10J/0C Calculate the enthalpy change DH from q(system) and the number of moles NaNO36. As shown in Figure, a gas within a piston-cylinder assembly undergoes a thermodynamic cycle consisting of three processes in series: Process 1-2: Compression with U 2 =U 1 . Process 2-3: Constant-volume cooling to p 3 =140 kPa,; V 3 =0.028 m^ 2 . Process 3 - 1 : Constant-pressure expansion with W 31 =10.5 kJ. For the cycle, W eycle =28.3 kJ . There are no changes in kinetic or potential energy. Determine (a) the volume at state 1, in m ^ 3 . (b) the work and heat transfer for process 1-2, each in kJ. (e) Can this be a power cycle? A refrigeration cycle? Explain.In this calorimetery experiment state the independent variable, dependent variable, and your control group. Here is rhe procedure of the experiment below: Gather the items to set up your calorimeter (coffee-cup, stir plate and stir bar, Vernier temperature probe, lid for coffee-cup) Pour 50.0 mL of DI water into the coffee-cup calorimeter. You will be preparing 50.0 mL of a 1.0 M solution of sodium nitrate solution. Using the Vernier temperature probe, record the initial temperature of your DI water. Weigh out the mass of sodium nitrate (4.25g) needed for your solution and pour it into the calorimeter. Immediately begin collecting temperature data. Repeat multiple times.