Directions: Draw the experimental set up for the determination of heat of an unknown metal. Any missing answer will result in DISLIKING your solutions.
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- When 0.6403 of g calcium bromide is dissolved in 75.00 mL water, the solution temperature increses by 1.07 °C. Calculate the enthalpy of dissolution (ΔHrxn) for calcium bromide, in kj/mol.(Assume constant pressure is, 41.84j/g. °C as the specific heat capacity of the solution, and a density of 1.00 g/ml). Write out the equation. I am confused on where to start with this problem.Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C How much heat is involved in taking 165.2 g of acetone from 14.7°C to 52.1°C?Estimate the thermal properties of a food with the following composition: carbohydrate 0.3%, protein 27.6%, fat 17.5%, ash 4.7%, moisture 49.9%. a. Specific heat is based on the Siebel equation = kJ / kg ° C. b. Specific heat is based on the Charm equation = kJ / kg ° C. c. Specific heat is based on the Heldman & Singh equation = kJ / kg ° C. d. Specific heat is based on the Choi & Okos equation = kJ / kg ° C. e. Heat conductivity is based on the equation Sweat = W / m ° C. f. Heat conductivity is based on the Choi & Okos equation = W / m ° C. g. Heat diffusivity based on the Choi & Okos equation = m² / s.
- A student determines the molar mass of a liquid unknown by the method used in thisexperiment. She found that the equilibrium temperature of a mixture of ice and water was1.0°C on her thermometer. When she added 12.3 g of her unknown sample to the mixture, thetemperature, after thorough stirring, fell to -4.0°C. She then poured off the solution through ascreen into a beaker. The mass of the solution was 93.4 g. Kf = 1.86°C/m What was the molality of the unknown solution? ______________ m How much unknown liquid was in the decanted solution? ______________ gHow much water was in the decanted solution? ______________ gWhat did she find to be the molar mass of the unknown liquid, assuming she made thecalculation properly?______________ gWhen two different liquids are mixed or when a gas or solid is dissolved in a liquid, bondsare broken between neighbouring molecules (or sometimes atom) in the feed materials,and new bonds are formed between neighbouring molecules (or ions) in the productsolution. i. Briefly distinguish between heat of solutions and standard heat of formation of solution.ii. Consider solid X is to be dissolved in solvent Y. If Δ?? °is the heat of formation of X(s),using the appropriate notations, write an equation to calculate the standard heat of formation of solution that contains 5 mol of X in 100 mol of Y at 25°C, relative to X and Y.The specific heat of an unknown liquid is determined using a sample of molybdenum (Mo) with a mass of 35.12g. The Mo is heated to 99.2OC in boiling water, and then transferred to 52.16g of unknown liquid whose temperature is 23.4OC. The final temperature of the Mo-unknown liquid system is 28.9OC. Calculate the specific heat of the unknown liquid. CMo = 0.251 J•g-1•OC-1
- 6.A fuel is burned with 50% excess air and the combustion characteristics of the fuel oil are similar to C12H26. Determine the ff. a) air fuel ratio b) volumetric (molal) analysis of the products of combustion.Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids Cations Cl--131.228 I--51.57 NO3--108.74 SO4-2-744.53 Ca2+-553.58 -748.1 -528.9 -743.07 -1797.28 W2 ∆G°f of water = -237.129 kJ/mol Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt).Observations (Rxn or No Rxn). S or support and R for Refute Cations Cl- I- NO3- SO4-2 Ca+2 help4.38 g of a gas (28.1 g mol–1) was dissolved in liquid water in a calorimeter with a calorimeter constant of 76.0 J K–1. Prior to mixing everything was equilibrated to 21.2 °C. The resulting solution with a mass of 23.4 g was observed to be at a temperature of -6.8 °C and have a specific heat capacity of 4.61 J g–1 K–1. Determine q per mole for this dissolution process. a. -5150 J/mol b. -1.94 × 104 J/mol c. 2.89 × 105 J/mol d. -3.39 × 105 J/mol e. 3.30 × 104 J/mol
- Extintion coeficient for Y is 12801. Calculate the concentration in % by mass of a solution containing 3.50 g of NaCl dissolved in 25000 mg of H2O. 2. Calculate the heat change of the combustion of 1.78 g benzoic acid (MM = 122 g/mol) in a constant bomb calorimeter. As measured, the temperature rises from 15.17°C to 28.52°C and the heat capacity of the bomb plus water is 5.7125 kJ/°C. What is the heat of combustion in kJ/mole?Name two characteristic physical properties that distinguish condensed from gas phases, and one which distinguishes solid from liquid phases. Discuss the differences for each property. Name one colligative property and by an equation (label all variables) and 1-2 sentences the physical meaning. Consider a balloon. What thermodynamic system does it represent? How does this system interact with the environment? Calculate the heat capacity at constant pressure of methane for all its contribution and the total value according to the equipartition theorem. What is a more realistic value at room temperature? Why?
