A 0.530-g sample of nonanedioic acid (C9H1604) is burned in a bomb calorimeter and the temperature increases from 24.00 °C to 26.73 °C. The calorimeter contains 1000 g of water and the bomb has a heat capacity of 793 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate AE for the combustion reaction per mole of nonanedioic acid burned. x 10^____ kJ/mol

A 0.530-g sample of nonanedioic acid (C9H1604) is burned in a bomb calorimeter and the temperature increases from 24.00 °C to 26.73 °C. The calorimeter contains 1000 g of water and the bomb has a heat capacity of 793 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate AE for the combustion reaction per mole of nonanedioic acid burned. x 10^____ 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

The standard molar enthalpy of formation of diborane, B₂H₁ (g), cannot be determined directly because the compound cannot be prepared by the reaction of boron and hydrogen. It can be calculated from other enthalpy changes, however. The following enthalpy changes can be measured. 4 B(s) + 3 O₂ (g) → 2 B₂O3 (s) A₁H° = -2543.8 kJ/mol-rxn H₂(g) + 1/2 O₂ (g) → H₂O(g) A, H = -241.8 kJ/mol-rxn B2 H6 (g) + 3 O2 (g) → B₂O3 (g) + 3 H₂O(g) A₁H° = −2032.9 kJ/mol-rxn a we will show how these equations can be added together to give the equation for the formation of B₂ H6 (g) from B(s) and H₂(g) in their standard states and determine the enthalpy of formation. The target reaction is 2 B(s) + 3 H₂(g) → B2H6 (g) Does Reaction 1 need to be used as is, or reversed? as is reversed The reaction is used as is because B(s) is a reactant in the target reaction and in Reaction 1. Correct b Does Reaction 1 need to be multiplied by a scaler? Choose a scaling number for Reaction 1. Target Reaction: 2 B(s) + 3…
The enthalpy (or heat) of combustion of acetone, (CH3)2CO, is - 1657.8 kJ. The reaction is (CH3)2CO (1) +4 0₂ (g) →3 CO₂(g) + 3 H₂O (g). Given the values of AH-393.5 kJ/mol for CO₂ (g) and AH-241.8 kJ/mol for H₂O(g), the calculated value of AH; for acetone O equals - 3563.7 kJ/mol O equals - 1022.5 kJ/mol O equals-248.1 kJ/mol O equals 1202.7 kJ/mol
Hydrazine, N2H4, is a liquid used as a rocket fuel. It reacts with oxygen to yield nitrogen gas and water. N2H4(l) + O2(g) → N2(g) + 2 H2O(l) The reaction of 6.50 g N2H4 evolves 126.2 kJ of heat. Calculate the enthalpy change per mole of hydrazine combusted. Express the answer in kJ/mol
What is the enthalpy change for the first reaction? CH4(g) + 1/2O2(g) → CH3OH(g) ΔH = CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ΔH = -806.5 CH3OH(l) + 3/2 O2 → CO2(g) + 2H2O(g) ΔH = -676.7
At constant volume, the heat of combustion of a particular compound is −3733.0 kJ/mol.−3733.0 kJ/mol. When 1.361 g1.361 g of this compound (molar mass=185.51 g/mol)(molar mass=185.51 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 8.567 ∘C.8.567 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?
Which one of the following statements is true? Which one of the following statements is true? Enthalpy is a state function. The enthalpy change of a reaction is the reciprocal of the ΔΔH of the reverse reaction. Enthalpy is an intensive property. H is the value of q measured under conditions of constant volume. The enthalpy change for a reaction is independent of the state of the reactants and products.
What mass (in g) of fructose, when having undergone complete combustion, will release 6.13 x 102 kJ of heat? C,H12O6 (s) + 602(g) → 6CO2(g) + 6H2O(1) AH = -2.83 x 10° kJ mol-1 A: 39.0 aldnl nom
A 3.59°C increase in temperature occurs when a 0.232 g sample of benzoic acid (C7H6O2) is combusted in a bomb calorimeter. A 1.81 °C increase in temperature occurs when a 0.303 g sample of citric acid (C6H8O7) is combusted in the same bomb calorimeter. The heat of combustion of benzoic acid is -26.37 kJ/g. What is the molar heat of combustion of citric acid? Reminder: Any heats of combustion will be negative since these are exothermic reactions.
MN.19.
The addition of hydroiodic acid to a silver nitrate solution precipitates silver iodide according to the reaction: AGNO3 (aq) + HI(aq) → AgI(s) + HNO3 (aq) When 50.0 mL of 5.00x10-2 M AgNO3 is combined with 50.0 mL of 5.00x10-2 M HI in a coffee-cup calorimeter, the temperature changes from 22.40 °C to 22.91 °C. Part A Calculate AHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and Cs = 4.18 J/(g·°C) as the specific heat capacity of the solution. Express the energy to two significant figures and include the appropriate units. HẢ Units Value ΔΗΚΗ rxn
Part A. In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJ Calculate the amount of energy released when one mole of hydrogen gas reacts. Consider this to be a positive value. kJ=___________ Part B. How much energy is released when 16.00 g of NH3(g) is made to react with an excess of steam to form HNO3 and H2 gases? Again, enter this as a positive value. HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJ kJ=___________
Part C Calculate the enthalpy change for the thermite reaction: 2Al(s) + Fe2 O3 (s)→2FE(s) + Al203 (s), AH° rxn = -850 kJ when 12.0 mol of Al undergoes the reaction with a stoichiometrically equivalent amount of Fe2O3. Express your answer to three significant figures and include the appropriate units.