When 50.0 mL of 2.00 M HCI is mixed with 50.0 mL of 2.00 M NaOH at 24.5°C, the solution temperature increases to 50.7°C. Calculate the AHrxn in kJ/mol HCl? Assume the density of the solution is 1.00g/mL, Ccal = 21.0J/°C & Cwater = 4.184 J/g*°C. Report your answer to 3 sf and remember to use the correct sign for AHxn- %3D

When 50.0 mL of 2.00 M HCI is mixed with 50.0 mL of 2.00 M NaOH at 24.5°C, the solution temperature increases to 50.7°C. Calculate the AHrxn in kJ/mol HCl? Assume the density of the solution is 1.00g/mL, Ccal = 21.0J/°C & Cwater = 4.184 J/g*°C. Report your answer to 3 sf and remember to use the correct sign for AHxn- %3D

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

When 50.0 mL of 2.00 M HCI is mixed with 50.0 mL of 2.00 M NaOH at 24.5°C, the solution temperature increases to 50.3°C. Calculate the AHrxn in kJ/mol HCI? Assume the density of the solution is 1.00g/mL, Ccal = 21.0J/°C & Cwater = 4.184 J/g*°C. Report your answer to 3 sf and remember to use the correct sign for AHexn- Your Answer: Answer units MacBook Air 80 88 DI DD F3 F6 F7 F8 F9 F10 F11 F2 F4 F5 # $ % & * 3 4 5 6 7 8 9. { W E T Y U [ G H J K C V N M command option command .. V
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.
Calculate the total enthalpy change (kJ) for the following reaction: H2O (s, 90 g, –10. oC) --> H2O (l, 90 g, 10. oC) (The specific heat capacity of ice is 2.0 J/g×oC; the specific heat capacity of liquid water is 4.2 J/g×oC; the enthalpy of fusion for H2O at 0 oC is 6.0 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
Help with the following question
Calculate the amount of salt in a commercial cold-pack containing ammonium nitrate (ΔHsol = + 25.7 kJ/mol) if the final temperature of the cold-pack is 3ºC. Assume that the initial temperature of water is 25ºC, mass of solution is 25 g and the specific heat of the solution is 4.184 J/g.K.
A student followed the procedure in this experiment , using 29.5 mL of 2.41 molar HCl and 31.5 mL of 2.41 molar NaOH , with both solutions having an initial temperature of 21.9 °C. After mixing , a maximum temperature of 31.0 °C is measured . The final mass of the mixture was found to be 62.201 grams . For this problem , assume the specific heat of the solution is 4.18 J/g °C. What is the heat transferred by this reaction, in Joules?
3.76 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g °C and the density of the water is 1.00 g/ mL). You can assume that the specific heat of the solution is the same as that of water.
Can someone verify my answers? I got: a) endothermic b)-1149.5 J c) 1149.5 J d)0.0117 mol e) 97704.05 J/mol
A student dissolves 11.0 g of sodium hydroxide (NaOH)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 21.0°C to 31.1 °C over the course of 6.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na (aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. - Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy A/, per mole of NaOH. O exothermic O…
dont hend written solution
Calculate the heat of neutralization (kJ/mole) for the reaction of 50.0 mL of 0.177 M potassium hydroxide with 100.0 mL 0.841 M sulfuric acid resulting in a temperature increase of 4.61 oC. Assume the solutions have a density of water and specific heat capacity of water, 4.184 J/(g⋅oC). The calorimeter is a perfect system with no heat loss. 2KOH + H2SO4 ⟶ K2SO4 + 2H2O Group of answer choices +34.4 kJ/mole -218 kJ/mole -34.4 kJ/mole +218 kJ/mole -2890 kJ/mole +654 kJ/mole -654 kJ/mole +2890 kJ/mole +109 kJ/mole -327 kJ/mole +327 kJ/mole -109 kJ/mole