When 5.93 g of potassium sulfate (K,SO4) is dissolved in 111 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 23.21 °C. Based on this observation, calculate q for the water and AH° for the process, assuming that the heat absorbed by the salt is negligible. K2SO4(s) 2K*(aq) + SO42- (aq) The specific heat of water is 4.184 J °C1 g1. Give the answers in kJ. kJ 9H20 = AH° = kJ Not submitted

When 5.93 g of potassium sulfate (K,SO4) is dissolved in 111 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 23.21 °C. Based on this observation, calculate q for the water and AH° for the process, assuming that the heat absorbed by the salt is negligible. K2SO4(s) 2K*(aq) + SO42- (aq) The specific heat of water is 4.184 J °C1 g1. Give the answers in kJ. kJ 9H20 = AH° = kJ Not submitted

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 system does 566566 kJ of work and loses 216216 kJ of heat to the surroundings. What is the change in internal energy, Δ?Δ⁢E, of the system? Note that internal energy is symbolized as Δ?Δ⁢U in some sources.
100. mL of 0.100M Ca(OH)2(aq) at 25.0 °C is combined with 100. mL of 0.100M HCl(aq) at 25.0 °C in a constant-pressure calorimeter. Given that the complete neutralization of 1.00 mol of Ca(OH)2 with HCl has ∆H = -110. kJ, and that the specific heat capacity and density of the resulting solution is ~equal to that of water, what is the temperature of the final solution?
Assuming that the specific heat of the solution is 4.18 J/(g⋅∘C)J/(g⋅∘C) and that the calorimeter itself absorbs a negligible amount of heat, calculate ΔHΔ� in kilojoules for the reaction K2O(s)+H2O(l)→2KOH(aq)
Trinitrotoluene (TNT) is a highly explosive compound. The thermal decomposition of TNT is described by the following chemical equation: The enthalpy change for the explosion of ammonium nitrate with fuel oil is –7198.00 kJ for 3 moles of NH4NO3. If ΔHrxn for the thermal decomposition of 2 moles of TNT is –20,306.00 kJ, how much TNT is needed to equal the explosive power of 1 mole of ammonium nitrate? g TNT
A quantity of 2.00×102 mL of 0.786 M HCl is mixed with 2.00×102 mL of 0.393 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.76°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions? H+(aq) + OH−(aq)→H2O(l) _____°C
In a coffee cup calorimeter, a student places 0.350 g of magnesium, followed by addition of 45.0 mL of 1.00 M hydrochloric acid. After the reaction took place, a the temperature rose from 21.5oC to 54.2oC. If the reaction solution has the same properties of water and the calorimeter constant is 5.38 J oC-1, how much heat was released from the reaction and what is the enthalpy of the reaction in kJ mol-1? Answer choices for heat released from reaction: -7.89 kJ, -4.12 kJ, -6.50 kJ, -5.66 kJ
Calculate the ΔH°rxn of the reaction in a bomb calorimeter: NaOH(s) → NaOH(aq) Given the following: Volume of solution = 100mL (when solid added to water) Concentration = 1M Mass of NaOH = 1.0359g Change in temperature = 2.5°C Specific heat capacity of solution = 4.184 J/°C Specific heat capacity of bomb calorimeter = 30 J/°C Molecular mass of NaOH = 40g/mol
A 1.22 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.47oC to 27.95oC. What is ΔH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)
When 7.31 g of cesium chloride (CSCI) is dissolved in 111 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 23.28 °C. Based on this observation, calculate q for the water and AH° for the process, assuming that the heat absorbed by the salt is negligible. CsCl(s) Cs+ (aq) + CI+ (aq) The specific heat of water is 4.184 J °C-1 g¹. Give the answers in kJ. kj 9H₂0 = ΔΗ° = kJ
A 0.588 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.706 kJ °C-1. If the temperature inside the calorimeter increased from 25.0 °C to 29.9 °C, determine ΔrU for this reaction in kJ mol-1 (with respect to C5H12). Do not worry about how realistic the final answer is. Express answer in 2 significant figures.
A 1.6 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.58oC to 27.95oC. What is ΔH
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 253. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 149. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 |kJ х10 significant digits. exothermic Is the reaction exothermic or endothermic? endothermic