Module A3_ Binary Solutions_ MSE318H1 S LEC0101 20211_Phase Transformations

2. Calculate the enthalpy change to be expected for the dissolution of NaOH ((s) and (aq) mean solid and aqueous) using Hess's Law: q + H*(aq) your class and NaOH(s) → NAOH(aq) НСІ culate the action. Use the enthalpy change for NaOH-HCI pair that your class measured in this experiment, and the data from the following table: Reaction* AH(kJ/mol) ½H2(g) + ½CI2(g) → HCI(g) - 92.3 Na(s) + ½O2(g) + ½H2(g) → NaOH(s) –426.8 Na(s) + ½CI2(g) → NaCI(s) – 411.1 H2(g) + ½O2(g) → H2O(1) - 285.8 HCI(g) → HCI(aq) -75.2 NaCI(s) → NaCI(aq) 4.0 NaOH(aq) + HCI(aq) → NaCl(aq) + H2O(1) *(g) = gas, (1) = liquid, (s) = solid, (aq) = aqueous %3D %3D %3D

7.46 g of ammonium persulfate is dissolved in 112.0 mL of water. Initially the temperature of the water is 14.78°C and after the ammonium persulfate has dissolved, the solution's temperature is now 21.50°C. What is the molar enthalpy of solution?

I need with blanks please

50.0 mL of 1.00 M HCl is mixed with 50.0 mL of 0.95 M KOH in a calorimeter with a caloriemeter constant (K cal ) of 17.3 J/^ C . A change in temperature was observed from 26.0C to 32.6^ ( C. What is the heat of reaction per mole of KOH? (Assume a solution density of 1.00g / (mL) and specific heat capacity of 4.18 J/g^ C .)

Consider a mixture of hexane and heptane as an ideal solution. In what proportion by mass should they be mixed to achieve the greatest ΔmixS?

When 4 grams of a certain compound is dissolved in 61 grams of water in a calorimeter, the temperature of the calorimeter changes from 25.00ºC to 26.98 ºC. Assuming that the specific heat capacity for the resulting solution is 4.184 J/(g oC), and the heat for this solvation is found as x kJ, what is the value of x?

In making homemade ice cream,  NaCl, MgCl2, and CaCO3 are the salts that are used to be dissolved in an ice-water mixture to lower the temperature of the mixture. The mixture will be then used to freeze ice cream. Which salt will be much more effective in lowering the temperature of the ice-water mixture considering that equal masses of each salt are to be compared? Use the basis of 100g (Kf,water = 1.86 K kg mol-1)

Given the following reaction:4 Fe(s) + 3 O2 (g) → 2 Fe2O3 (s) ΔH = -1648 kJ52.0 g of Fe (MM = 55.845 g/mol) are reacted as above in 1.000 x 103 g of water (MM = 18.02, ΔHFUSION = 6.01 kJ/mol, ΔHVAP = 40.65 kJ/mol, specific heat = 4.18 J/(g C) that is at 20.0 °C. What will the final temperature of the water be?Select one:367 112 20.1 91.8 100

Suppose that 125 mL of 0.1125 M HCI is reacted with 155 mL of 0.1010 M NaOH in a coffee-cup calorimeter. HCl(aq) + NaOH H20(1) + NaCl(aq) -56 KJ mol ΔΗ If the initial temperature of the mixture is 22.1°C, calculate the final temperature of the mixture given the following information. Ssolution = 4.1 g.°C %3D Dsolution = 1.02 mL 25.5 °C 24.3 °C 22.8 °C O 19.8 °C

Would the amount of heat absorbed by the dissolution as given below appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.     When solid ammonium nitrate dissolves in water, the solution becomes cold. This is the basis for an “instant ice pack” (see image). When 3.21 g of solid NH4NO3 dissolves in 50.0 g of water at 24.9 °C in a calorimeter, the temperature decreases to 20.3 °C.Calculate the value of q for this reaction and explain the meaning of its arithmetic sign. State any assumptions that you made.

The combustion of propane gas leads to formation of carbon dioxide and water by the following equation:  C3H8(g) + 5 O2(g) -> 3 CO2(g) + 4 H2O(l) The standard enthalpy for the reaction delta H° = -2220.0 kJ. If 2.84 x 10^3 of kJ of heat are evolved, what volume of CO2 gas in Liters is produced if this reaction occurs at a pressure of 748 tote and 71°C?

1 (a) Does doubling the volumes of acid and base double the amount of heat? 1 (b) Does doubling the concentrations of acid and base double the amount of heat? 2 (a) What happens when different amounts of acid and base are used? What happens when sulfuric acid is substitutted for hydrochloric acid?

Given the following reaction: 4 Fe(s) + 3 O2 (g)  →  2 Fe2O3 (s)  ΔH = -1648 kJ 52.0 g of Fe (MM = 55.845 g/mol) are reacted as above in 1.000 x 103 g of water (MM = 18.02, ΔHFUSION = 6.01 kJ/mol, ΔHVAP = 40.65 kJ/mol, specific heat = 4.18 J/(g C) that is at 20.0 °C.  What will the final temperature of the water be?

Given the following reaction: 4 Fe(s) + 3 O2 (g) → 2 Fe2O3 (s) ΔH = -1648 kJ 52.0 g of Fe (MM = 55.845 g/mol) are reacted as above in 1.000 x 103 g of water (MM = 18.02, ΔHFUSION = 6.01 kJ/mol, ΔHVAP = 40.65 kJ/mol, specific heat = 4.18 J/(g C) that is at 20.0 °C. What will the final temperature of the water be? Select one: 100 367 91.8 112 20.1

is number 9 correct?

At 768 oC, Keq = 0.0725 for the reaction: NO(g) + 1/2 Cl2(g)  NOCl(g) (a) What is the value of Keq for the reaction NOCl(g)  NO(g) + 1/2 Cl2(g)?Keq =  .(b) What is the value of Keq for the reaction 2 NO(g) + Cl2(g)  2 NOCl(g)?Keq =  .(c) What is the value of Keq for the reaction 2 NOCl(g)  2 NO(g) + Cl2(g)?Keq =  .

A 2C3H18(1) + 2502(g) = 16CO2(g) + 18H20(1) B CO2(g) + 2H20(g) = CO2(g) + 4H2(g) C 3CO(g) + Fe,03(s) = 3CO2(g) + 2Fe(s) Which of these processes energetically favors the products A only B and C only А, В and C A and C only

Given the standard enthalpy changes for the following two reactions:(1) N2(g) + 2O2(g) -> 2NO2(g)...... ΔH° = 66.4 kJ(2) 2N2O(g) -> 2N2(g) + O2(g)......ΔH° = -164.2 kJwhat is the standard enthalpy change for the reaction:(3) 2N2O(g) + 3O2(g) -> 4NO2(g)......ΔH° = ?_____ kJ

A 75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC.   Then the reaction is proceeded and the final temperature is reached to 28.000 oC.  Calculate the heat of reaction in kJ / mole. Hint: Treat this mixture as a diluted solution. CP of H2O(l) = 4.184 J / g oC D of H2O = 0.988 g/ mL.

A 75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC.   Then the reaction is proceeded and the final temperature is reached to 28.000 oC.  Calculate the heat of reaction in kJ / mole. Hint: Treat this mixture as a diluted solution. CP of H2O(l) = 4.184 J / g oC D of H2O = 0.988 g/ mL.  a. -37.3 kJ / moleb. -55.9 kJ/ molec. 124 kJ / moled. -124 kJ / mole

The quantity of 83.0 g of potassium iodide (KI) is added to water to give a solution with a mass of 150. g. Assume that this solution is very dilute and thus has the same heat capacity as water. The dissolution reaction and the associated heat for potassium iodide is KI (s) -→ K+(aq) + I-(aq) qrx = DHrx = +20.3 kJ. Calculate the change in the temperature of the solution.

7) ( Use the following data to calculate the enthalpy of solution of lithium chloride. H, for solid lithium chloride = -408.7 kJ/mol, H, for hydration of lithium chloride = -445.6 kJ/mol.