You mix 208 ml of 0.291 M LIOH with 208 ml of 0.536 M HF in a coffee-cup calorimeter, and the T of the solution rises from 21.0°C to 26°C (what does that mean T increasing?). What is the enthalpy of reaction/mole of LiF (AH in kJ/mol??)? Assume density of the solutions are all 1.00 g/ml, and the c of the solutions are 4.2 J/gK. Use the correct sign (+ vs -). Enter to 1 decimal place with the correct sign (+ or -).

You mix 208 ml of 0.291 M LIOH with 208 ml of 0.536 M HF in a coffee-cup calorimeter, and the T of the solution rises from 21.0°C to 26°C (what does that mean T increasing?). What is the enthalpy of reaction/mole of LiF (AH in kJ/mol??)? Assume density of the solutions are all 1.00 g/ml, and the c of the solutions are 4.2 J/gK. Use the correct sign (+ vs -). Enter to 1 decimal place with the correct sign (+ or -).

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...

See similar textbooks

Similar questions

Please determine the enthalpy (in kJ/mol) of the balanced thermochemical equation when 2.15 g of NaOH(s) are mixed with 25.4 mL of 1.00 M HCl. Before reaction the HCl was at an initial temperature of 20.29o At the completion of the reaction the temperature increased to 25.14oC (Hint: This calculation is similar to the lab calcs.)
A student followed the procedure in this experiment, using 29.5 mL of 1.66 molar HCl and 31.5 mL of 1.66 molar NaOH, with both solutions having an initial temperature of 22.1 oC. After mixing, a maximum temperature of 30.7 oC is measured. The final mass of the mixture was found to be 63.194 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format.
When 17.98 g of calcium chloride (CaCl2) is dissolved in 681.87 g of water in a coffee-cup calorimeter at 26.4°C, the temperature increased to 28.4 °C. Assuming that the specific heat of the mixture is the same as the specific heat of pure water (4.184 J/g-°C), calculate the AH (in kJ/mol CaCl2) in the dissolution process. MW of CaCl2 = 110.9g/mol CaCl2 (s) →→ Ca+2 (aq) + 2 CI¯ (aq) Show your complete solution. Express your answer in two decimal places.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
In a coffee cup calorimeter, 50.0 mL of 0.124 M AgNO3 and 50.0 mL of 0.124 M HBr are mixed. The following reaction occurs. Ag*(aq) + Br (aq) → AgBr(s) If the two solutions are initially at 23.92°C, and if the final temperature is 25.17°C, calculate AH for the reaction in kJ/mol of AgBr formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-1g-¹. kJ/mol
Macmillan Learning In a constant-pressure calorimeter, 55.0 mL of 0.330 M Ba(OH), was added to 55.0 mL of 0.660 M HCI. The reaction caused the temperature of the solution to rise from 24.25 °C to 28.75 °C. If the solution has the same density and specific heat as water (1.00 g/mL. and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H₂O
true or false? 3 The enthalpy changes for the reaction CO₂(g) + 3H₂(g) CH3OH(g) + H₂O(g) exceeds -52 kJ/mol.
Consider an endothermic reaction that takes place in 303 mL of solution. If the reaction requires 4,468 J of energy and the initial temperature of the solution is 26.7, what will the final solution temperature be? (3 sf) The density of solution is 1.00 g/mL and the specific heat of the solution is the same as that of water.
MN.19.
The answer is 44.8 kJ/mol. Show the solution how to get 44.8 kJ/mol.
8
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