QUESTION 14 When 33.42 grams of fictional compound X is added to water to make 398.4 grams of solution, the temperature increases from 24.83 °C to 54.50 °C. What is the heat of solution for compound X given that the molar mass of compound X is 71.62 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C. -8.305 kJ/mol -105.9 kJ/mol O -49.41 kJ/mol O 105.9 kJ/mol 49.41 kJ/mol

QUESTION 14 When 33.42 grams of fictional compound X is added to water to make 398.4 grams of solution, the temperature increases from 24.83 °C to 54.50 °C. What is the heat of solution for compound X given that the molar mass of compound X is 71.62 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C. -8.305 kJ/mol -105.9 kJ/mol O -49.41 kJ/mol O 105.9 kJ/mol 49.41 kJ/mol

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

A cold pack contains 134.4 g of water and 40.7 g of ammonium nitrate. What will be the final temperature of the activated cold pack, if the initial temperature is 26.8 °C? (Assume that the specific heat of the solution is the same as that for water, 4.184 J/g °C and no heat is lost). The heat of solution of ammonium nitrate is 25.4 kJ/mol. Please do not include units in your answer.
A chemist dissolved an 10.8-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 23.9°C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g - °C. %3D =Db Calculate the heat of solution for KOH in kJ/mol. kJ/mol heat of solution =
4. In a coffee-cup calorimeter, 3.20 g of NH4NO3 is mixed with 86.00 g of water at an initial temperature of 23.53°C. After dissolution of the salt, the final temperature of the calorimeter contents is 21.32°C. Assuming the solution has a heat capacity of 4.184 J/g °C and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Ices] A 21.0 g sample of pure iron at 85 °C is dropped into 66 g of water at 20. °C. What is the final temperature of the water-iron mixture? The specific heat of water is 4.184 J/g °C. The specific heat of iron is 0.45 J/g °C. Final temperature °C
When 2.105 g of NH4NO3 (molar mass is 80.05 g/mL) is added to 100.0 mL of water at 25.05C, the final temperature of the water is 23.44C. What is the molar heat of solution (H) of NH4NO3 in kJ/mol?the density of water is 1.00 g/mL and the specific heat is 4.184 J/gC:q = mwater x Cwater x Twater
A particular sample of cold graphite at 10.20 °C was added to 988.5 g of water at 25.31 °C in a constant pressure calorimeter. If the final temperature of the graphite and water was 25.17 °C, what was the mass of the graphite sample? Assume no heat was lost to the surroundings. The specific heat for water is 4.184 J/g•°C and the specific heat for this graphite is 0.7069 J/g•°C.
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.
A chemist dissolved an 14.2-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 30.5 ∘C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g⋅°C. ?= kJ Calculate the heat of solution for KOH in kJ/mol.
In a coffee cup calorimeter with a heat capacity of 21.5 J/ºC, 225 mL of 0.20 M KOH at 22.3 ºC neutralizes 225 mL of 0.20 M HCl at 22.3 ºC. After the reaction occurs, the temperature of the resulting mixture is 29.2 ºC. The density of the final solution is 1.00 g/mL and the specific heat is 4.18 J/g°C. Calculate the Heat of neutralization of KOH.
The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
A solution is made by mixing 232.0 mL of ethanol initially at 12.7 ∘C with 232.0 mL of water initially at 22.5 ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C ?f= ∘C
The enthalpy of solution (∆H) of KOH is -57.6 kJ/mol. If 2.26 g KOH is dissolved in enough water to make a 150.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g･°C and the density of the solution is 1.02 g/mL).