4. 56.0 ml of 1.5 M HCl is mixed with 68.5 mL of 1.33 M NAOH in a calorimeter cup (C= 55.35 J/ C) If the initial temperatures of both solutions before mixing is 21.78°C determine the final temperature of the combined solutions after the reaction takes place. Step 1: Determine the moles of HCl and NaOH present and clearly identify the limiting reactant. Show all calculations. Step 2: Use the limiting reactant and AH,n=-57.62 kJ/mole to determine the heat released by the reaction. Show all calculations. Step 3: Use the heat you determined in Step 2 to calculate the temperature change using m.olution X Celution X AT the equation: Ca x AT. Assume the solution has the same density and specific heat as pure water. Show all calculations. Step 4: Assuming the initial temperature of the two solutions is 21.78 C, determine the final temperature of the total solution. Show all calculations.

4. 56.0 ml of 1.5 M HCl is mixed with 68.5 mL of 1.33 M NAOH in a calorimeter cup (C= 55.35 J/ C) If the initial temperatures of both solutions before mixing is 21.78°C determine the final temperature of the combined solutions after the reaction takes place. Step 1: Determine the moles of HCl and NaOH present and clearly identify the limiting reactant. Show all calculations. Step 2: Use the limiting reactant and AH,n=-57.62 kJ/mole to determine the heat released by the reaction. Show all calculations. Step 3: Use the heat you determined in Step 2 to calculate the temperature change using m.olution X Celution X AT the equation: Ca x AT. Assume the solution has the same density and specific heat as pure water. Show all calculations. Step 4: Assuming the initial temperature of the two solutions is 21.78 C, determine the final temperature of the total solution. Show all calculations.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4.
When 6.30 g sample of solid potassium hydroxide (MM= 56.11g/mol) is dissolved in 101.00 g of water (at 21.2 degrees Celsius) the temperature of the resulting solution is 38.8 degrees Celsius. What is the AH for this dissolution reaction? Assume the specific heat of the solution is the same as water. Only include the numerical value not units or labels.
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC. After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures. What is the heat transferred by this reaction, in Joules?
Chemistry 14) A 60.0 mL quantity of 0.80 M HCI is mixed with 60.0 mL of 0.80 M KOH in a constant pressure calorimeter with negligible heat capacity. If the initial temperatures of both solutions are equal to 20.24°C. Calculate the heat change of the neutralization reaction if the final temperature of the mixture is 30.0°C. Assume that the densities and specific heats of the solutions are the same as those of water (1.00 g/mL and 4.184 J/g °C, respectively). Note: this point is worth 10 points. A) + 4900.3 J B)-1171.2 J C)-2450.15 J D)-4900.3 J
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MN.19.
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1. Draw an enthalpy diagram for the reaction between calcium carbide (CaC2) and water to form acetylene (C2H2) gas AH rxn = -712.8 kJ. 2. Calculate the enthalpy of solution if 0.4 mol of salt are dissolved in a calorimeter containing 100.0 g of water (SH2O=4.184 J/g°C, Ccal=15.0 J/°C) if T¡ = 25.0°C and Tf = 22.7°C
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The overall reaction in commercial heat packs can be represented as 4Fe(s) + 302(g) →2Fe₂O3 (8) AH = -1652 kJ a. How much heat is released when 2.20 mol iron is reacted with excess O₂? kl released b. How much heat is released when 1.83 mol Fe2O3 is produced? kJ released c. How much heat is released when 2.20 g iron is reacted with excess O₂? kJ released d. How much heat is released when 11.8 g Fe and 2.61 g O2 are reacted? Submit Answer [Review Topics] kl released Retry Entire Group [References] 8 more group attempts remaining
Consider the reaction 2H2+O2⟶2H2OΔ?rxn=−484 kJ Which answer best describes the transfer of heat that occurs when 1.40 mol H2 reacts? 678 kJ absorbed 484 kJ released 339 kJ released 678 kJ released 484 kJ absorbed 339 kJ absorbed