The molar heat capacity (Cpm (T)) for N2 is given by, P,m Cp.m (T)=(27.0+5.9×10T-0.34×10“T²)J mol' K Calculate AH when heating 1 mol of N2 from 25-125°C.
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- To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. 1. Calculate the experimental ΔHrxn (in kJ/mol) for the reaction between MgO andHCl.2. If the theoretical ΔHrxn of the reaction between MgO and HCl is -1349 kJ/mol, calculate the %error.A laboratory animal exercised on a treadmill, which, through pulleys, raised a mass of 200 g through 1.55 m. At the same time, the animal lost 5.0 J of energy as heat. Disregarding all other losses and regarding the animal as a closed system, what is its change in internal energy?A sample of a serum of mass 26.6 g is cooled from 290 K to 275 K at constant pressure by the extraction of 1.05 kJ of energy as heat. Calculate q and ΔH and estimate the heat capacity of the sample. report here the heat capacity = ________ J/k/g. 3 sig. number
- 2.8 g of a solid was dissolved in 51.4 g of a basic solution in a calorimeter with a calorimeter constant of 37.0 J K–1 with all substances initially at 81.5 °C.The resulting solution was observed to be at a temperature of 59.8 °C and have a heat capacity of 3.81 J g–1 K–1.Determine q for the dissolution process.Benzoic acid of mass 1.40 g is reacted with oxygen in a constant volume calorimeter to form H2O(l) and CO2(g) at 298 K. The mass of the water in the inner bath is 1.40×103g. The temperature of the calorimeter and its contents rises 2.84 K as a result of this reaction. Part A Calculate the calorimeter constant. The standard enthalpy of combustion of benzoic acid at 298 K is −3227 kJ⋅mol−1. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1.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.
- 1. Calculate the standard enthalpy of formation of C10H10. Its standard enthalpy of combustion is shown by the equation: 2C10H10 (l) + 25O2 (g) → 20CO2 (g) + 10H2O (l) ∆H = 10,314 KJ/mol The standard heat of formation (KJ/mol) at 298.15oC : CO2 = -393.5 ; H2O(l) = -285.8 2. Determine ΔG° at 298.15K for the reaction: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Given that ΔH° = -1648 kJ ; ΔS° = -549.3 J/K 3. In the picture, Find the the ∆H°rxn if ∆G°rxn is 420 kJ/mol and ∆S°rxn is -143 J/mol*kAt low temperatures the heat capacity of Ag(s) is found to obey the Debye law Cp,m = aT3, with a = 1.956 × 10−4 J K−4 mol−1. Determine Sm(10 K) − Sm(0) for silver.a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
- At constant pressure and 25C, what is enthalpy for the reaction: 2C2H6 + 7O2 -> 4CO2 + H2O, if the complete consumption of 12g of C2H6 liberates - 700kJ of heat energy? (-3508 kJ)The complete combustion of solid fumaric acid, HOOCCH=CHCOOH, in a bomb calorimeter released 1333 kJ mol -1 of heat at 298 K. Calculate (a) the internal energy of combustion, (b) the enthalpy of combustion . (c) Usetabulated values for the standard enthalpy of formation of water and carbon dioxide to calculate the enthalpy of formation of solid fumaric acid.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.