The combustion of 1.876 g of propanol (C,H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.38 K. The heat capacity of the bomb calorimeter is 14.38 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. AH = kJ/mol TOOLS

The combustion of 1.876 g of propanol (C,H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.38 K. The heat capacity of the bomb calorimeter is 14.38 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. AH = kJ/mol TOOLS

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 methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released, as shown in the combustion reaction. CH, OH(g) + O₂(g) → CO₂(g) + 2H₂O(1) AH = -764 kJ Based on the balanced thermochemical reaction, how much heat is produced when 25.7 g of methanol reacts with 39.9 g of oxygen? heat: Which reactant is limiting? methanol oxygen kJ
The enthalpy of combustion for methanol (CH3OH) is -715.0 kJ/mol. What mass of methanol is needed to produce 170J of energy? Group of answer choices 7.62x10-3 g 22.3 g 1.58g 5.22x10-4 g 3.02g
A chemist carefully measures the amount of heat needed to raise the temperature of a 854.0 mg sample of a pure substance from -6.7 °C to 16.2 °C. The experiment shows that 2.72 1 of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. 0.P X
5. A 1.500-g sample of a hydrocarbon is placed in a bomb calorimeter and undergoes combustion. The temperature of the calorimeter rises from 20.00°C to 23.55°C. If the calorimeter has a heat capacity of 40.3 J/°C, what is the heat of combustion (qv) for this hydrocarbon in kJ/g? 6. The heat of sublimation for iodine is 62.4 kJ/mol, at 25°C and 1.00 atm. What is AE for the sublimation of iodine (shown below) under these conditions? 2 (s) F 2 (g) volsd 7. A bomb calorimeter with heat capacity of 1.500x103 J/°C was used to study combustion of terbium (Tb) in excess oxygen: 4 Tb (s) + 3 O2 (g) →2 Tb2O3 (s) When 1.000-g of terbium was burned, a temperature increase of 3.908°C was observed. What is the AE for the reaction, in kJ/mol of Tb2O3?
Please don't provide handwriting solution
4.A 10. g cube of copper at a temperature T₁ is placed in a calorimeter containing 10. g of water at a temperature T₂. If T₁ > T₂, which of the following is true of the system when it has attained thermal equilibrium? 2 (The specific heat of copper is 0.385 J/(g°C) and the specific heat of water is 4.18 J/(g°C).) The temperature of the copper changed more than the temperature of the water. B) The temperature of the water changed more than the temperature of the copper. C) The temperature of the water and the copper changed by the same amount. D) The relative temperature changes of the copper and the water cannot be determined without knowing T₁ and T₂.
A chemist carefully measures the amount of heat needed to raise the temperature of a 442.0 g sample of a pure substance from -0.6 °C to 11.2 °C. The experiment shows that 725. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. [J.8 1 ∙K - 1 x10 X Ś
Enthalpy is the energy absorbed or released when a chemical change occurs. Assume you have the following thermochemical reaction: 2H2Sig) + 3021g) -> 2SOzig) + 2H2Oig AH = -1036 KJ How much energy is absorbed or released when 19.6 g of hydrogen sulfide (H,S) is burned? Is this an exothermic or endothermic reaction? Show all work for full credit.
1 . A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.290 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol･°C. 2. 3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 15.41°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･°C and the density of the solution is 1.20 g/mL). 3. Using the equations 2 Fe (s) + 3 Cl₂ (g) → 2 FeCl₃ (s) ∆H° = -800.0 kJ/mol Si(s) + 2 Cl₂ (g) → SiCl₄ (s) ∆H° = -640.1 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s) 4. A sample of 2.30 g of potato chips was burned in a calorimeter. The calorimeter was calibrated to have a heat capacity of 6.94 kcal/°C. The heat released caused the temperature of the calorimeter to increase 1.75°C. Calculate the food caloric content of…
please dont round along the way to solving
1. Hydrochloric acid is neutralized with potassium hydroxide in the following reaction HC1 (aq) + KOH (aq) --> KC1 (aq) + H₂O (1) DH° = -5 557 J/mol 40.00 mL of 1.500 mol/L solutions of both reactants, at 23.32 °C are mixed in a calorimeter. What is the final temperature of the mixture? Assume that the density of both solutions is 1.000 g/mL. Also assume that the specific heat capacity of both solutions is the same as the specific heat capacity of water (4.184 J/g °C).
A piece of lead (mass = 2.85 g) at 10.3 C is placed in a Styrofoam coffee cup containing 7.55 mL of water at 52.3 C. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature should be? The specific heat capacity of lead = 0.128 J/g°C and water = 4.18 J/g°C. density of water = 1.00 g/mL