4.41 g of MgS04 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 M9SO4. (The specific heat of water is 4.18 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. |kJ/mol

4.41 g of MgS04 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 M9SO4. (The specific heat of water is 4.18 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. |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

Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2 M(s) +0,(g) → M,0,(s) For this reaction, AHn = -5.919 kJ/mol and ASan = 12.37 J/(mol·K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AGixn = kJ/mol
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
Consider the following reaction at 25°C: 3 Ni(s) + N²(g) + 3 H2O(g) → 3 NiO(s) + 2NH:(g) where K = 6.74 x 104 At what partial pressure of ammonia will one be able to get out 11.5 kJ/mol of Gibbs free energy from this reaction when the rest of the mixture contains 57.6 g NiO, 182.3 g Ni, 8.54 atm of nitrogen gas, and 10.07 atm of water vapor? (Enter the partial pressure using two significant figures.)
An experiment was conducted to find the heat of neutralisation in an acid - basereaction.A solution was made by dissolving 3.79g of barium hydroxide in 100 mL of water. 30.0 mL of this barium hydroxide solution was reacted with 27.0 mL of a 0.400 mol L-1solution of nitric acid. The heat of neutralisation was calculated to be 51.7 kJ mol-1. Calculate the temperature change and the resultant pH of the solution
You add some of the white crystals to a small test tube filled with water. The water in the test tube was initially at room temperature (25˚C). Once the crystals were added and the tube was stirred, the temperature of the solution decreased to about 15˚C and all of the crystals dissolved. what is the change in Gibbs free energy (∆G) for this process?
What is the enthalpy change when 8.20 moles ammonium chloride form in the following equation? N2 (g) + 4 H2 (g) + Cl2 (g) --> 2 NH4Cl (s) Delta H = – 628.8 kJ a. – 2.58 x 103 kJ b. – 1.29 x 103 kJ c. + 314.4 kJ d. – 314.4 kJ e. – 628.8 kJ f. – 5.16 x 103 kJ g. none of these d. – 314.4 kJ
4.71 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.
5.61 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, 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.
How much heat is gained (in Joules) by the water where a chemical reaction takes place in 100 mL aqueous solution and has a temperature increase of 10 C?
A 75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC. Then the reaction is proceeded and the final temperature is reached to 28.000 oC. Calculate the heat of reaction in kJ / mole. Hint: Treat this mixture as a diluted solution. CP of H2O(l) = 4.184 J / g oC D of H2O = 0.988 g/ mL.