When 51.96 grams of fictional compound X is added to water to make 348.0 grams of solution, the temperature increases from 26.45 °C to 33.41 °C. What is the heat of solution for compound X given that the molar mass of compound X is 92.68 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C. O 10.12 kJ/mol O 18.06 kJ/mol O-18.06 kJ/mol O -10.12 kJ/mol O 2.680 kJ/mol

When 51.96 grams of fictional compound X is added to water to make 348.0 grams of solution, the temperature increases from 26.45 °C to 33.41 °C. What is the heat of solution for compound X given that the molar mass of compound X is 92.68 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C. O 10.12 kJ/mol O 18.06 kJ/mol O-18.06 kJ/mol O -10.12 kJ/mol O 2.680 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

When 54.29 grams of fictional compound X is added to water to make 341.3 grams of solution, the temperature increases from 20.29 °C to 83.39 °C. What is the heat of solution for compound X given that the molar mass of compound X is 154.77 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C. a -256.6 kJ/mol b 15.50 kJ/mol c 256.6 kJ/mol d -90.02 kJ/mol e 90.02 kJ/mol
A 33.6-g piece of silver initially at 46.5 °C is submerged into 162.4 g of water at 12.3 °C. What is the final temperature of the metal once the metal and water reaches thermal equilibrium? The specific heats of silver and water are 0.235 J/g·°C and 4.18 J/g·°C, respectively. 29.4 °C 10.4 °C 11.0 °C 12.7 °C 21.0 °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
When 30.87 grams of fictional compound X is added to water to make 438.9 grams of solution, the temperature increases from 26.23 °C to 62.34 °C. What is the heat of solution for compound X given that the molar mass of compound X is 130.58 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C. -280.2 kJ/mol 280.2 kJ/mol -66.24 kJ/mol 4.649 kJ/mol 66.24 kJ/mol
When 40.00 grams of fictional compound X is added to water to make 236.0 grams of solution, the temperature increases from 19.05 °C to 63.46 °C. What is the heat of solution for compound X (in kJ/mol) given that the molar mass of compound X is 73.87 g/mol. Assume the specific heat capacity of the solution is 4.18 J/g°C.
How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.
What is the heat capacity of 2.63 mol of liquid water? How many kJ of heat are needed to raise the temperature of 2.60 kg of water from 41.1 oC to 70.9 oC?
If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?
(please type answer no write by hand)
The temperature of 34.7 g H2O changes from 27 °C to 53 °C. What is the heat associated with this change? Is heat flowing into or out of the water? How do you know?
A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 156 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 degrees Celsius. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water. Enter your answer in kilojoules per mole of compound to three significant figures.
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).