3. Mixing 1.00 mL of 1.00 M HNO, and 1.00 mL of 1.00 M KOH causes the temperature of the two at 21.3°C to become 31.2°C. Calculate the heat of neutralization.
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- Adding table salt to water elevates its boiling temperature and speeds up the cooking process (although to what extent depends on how much the boiling point is increased). If one tablespoon of table salt (17 g, 0.291 mol) is added to 2 L of water (Kb = 0.512 °C m-1), what is the boiling point elevation of that water?Please ASAP. Thank you. Calculate the equilibrium potential for Na+, K+, Ca++, and Cl- ions? Na=+58.08; K= -80; Ca=+30.75; Cl=-63.5 Na=+58.08; K= +80; Ca=+30.75; Cl=-63.5 Na=+58.08; K= -80; Ca=+30.75; Cl=-57.24 Na=-58.08; K= +80; Ca=+30.75; Cl=-63.5 Na=+58.08; K= -80; Ca=-30.75; Cl=-63.56 . Enthalapy of solution For NH4No3 and MgSO4
- If 1000 L of gasoline has spilled into the street (MW=117 g/mol, density=0.7 g/mL which is true for octane) then firefighters add a lot of a material that dissolves into it that reduces the vapor pressure (liquid octane doesn’t burn, only the vapors). The firefighters put 500 kg of a material into the gasoline and reduced its vapor pressure from the pure partial pressure of 10.0 kPa down to 8.0 kPa. What is the molecular weight of the material that was added? (hint: use Raoult’s Law, which relates changes in pressure to the mol fractions.Part A. Heat of Neutralization Table 1. Heat of neutralization data Sample 1 Sample 2 [1] Volume of HCI (mL) 50.2 50.2 [2] Temperature of HCI (°C) 24.8 24.3 [3] Volume of NaOH (mL) 49.8 49.9 [4] Temperature of mixture after reaction (°C) 31.8 31.0 Part B. Enthalpy of Solution of Salts Table 2. Enthalpy of solution of salts data FON*HN MgSO4 [1] Mass of salt (g) 2.000 2.001 [2] Volume of DI water (mL) 50.1 50.1 [3] Temperature of DI water (*C) 25.0 24.5 [4] Temperature of mixture after dissolution (*C) 22.0 31.2 Part C. Specific Heat of a Metal Enter the number corresponding to the identity of the metal. 1. Zinc 2. Aluminum 3. Steel 4. Tin [1] Mass of metal (g) 19.985 [2] Volume of DI water (mL) 49.8 [3] Tinitial metal ("C) 97.0 [4] Tinitial water (°C) 24.7 [5] Tinal of mixture after addition of metal (°C) 25.92 CHEMICAL POTENTIAL [6] Calculate the difference in slope of the chemical potential against temperature on either side of (a) The freezing point of water (b) The boiling point of water Data: Afus H=6.01 x 103 J mol-1 AvapH =40.6 x 103 J mol-1 Which state function does the slope represent? Why is the slope steeper for evaporation?
- What is a marine calcifier and what are the effects of acidification on marine calcifiers?2.28(b) Set up a thermodynamic cycle for determining the enthalpy of hydration of Ca?+ ions using the following data: enthalpy of sublimation of Ca(s), +178.2 kJ mol-1; first and second ionization enthalpies of Ca(g), 589.7 kJ mol-1 and 1145 kJ mol¬1; enthalpy of vaporization of bromine, +30.91 kJ mol-1; dissociation enthalpy of Br,(g), +192.9 kJ mol-1; electron gain enthalpy of Br(g), –331.0 kJ mol-1; enthalpy of solution of CaBr,(s), –103.1 kJ mol-'; enthalpy of hydration of Br¯(g), –337 kJ mol¬!.Calculate the lattice enthalpy(nearest integer value) in kJmol-1 of LiF, given that ,enthalpy of sublimation of lithium is 155.3kJ mol-1 (i) ;dissociation of 1/2 mole of F2 is 75.3kJ (ii) ;ionization enthalpy of lithium is 520kJ mol-1 (iii) electron gain enthalpy of 1 mole of F(g) is -333k (iv) AfH overall is -594kJ mol-1 (v)
- Calculate the enthalpies of solution of barium sulphate in electron volts (eV), using the following data. Express your final answer to 2 deçimal places only. Enthalpy of hydration of 2+ Ba = -1,364 kJ/mol. Enthalpy of lattice formation of BaSO= -2,474 kJ/mol. Enthalpy of hydration of So, = -1,004 kJ/mol. %D 42- %3D 4.When 80 mg of an unknown white powder found at a crime scene is dissolved in 1.42 mL of ethand density = 0.789g/mL, normal freezing point -114.6 °C, Kf = 1.99 °C/m), the freezing point is lowere -115.6 °C. Which of the following substances could be responsible for this freezing-point depressio (assume the powder is a nonelectrolyte) Show all the work you used to determine the answer. a) meta-tyramine (C8H₁₁NO: MM = 137.182 g/mol) b) sucrose (C12H22O11: MM = 342.2965 g/mol) c) cocaine (C17H21NO4: MM = 303.353 g/mol) d) fructose (C6H12O6: MM = 180.16 g/mol) e) codeine (C18H21 NO3: MM = 299.364 g/mol) of been uov bluow 10cl doum woh (3Certain amount of pure charcoal (carbon) has to be burnt with supplied natural air. Process engineer allowed exact amount of air required to burn the entire charcoal completely to carbon dioxide. Carbon has no reaction with nitrogen gas present in the air. In the reaction outlet if 50 kg of carbon dioxide gas was found, calculate the amount of charcoal and air used. (12C, 16O, 14N).