lpacellus_engine.html?ClassID=1246112631#Student Orie.Using the data below, calculate the enthalpy for thedecomposition of sodium bicarbonate.2NaHCO3(s) → Na,CO3(s) + H2O(g) + CO2(g)Compounds S (J/mol-K) AHF° (kJ/mol)NaHCO,(s)Na,CO,(s)CO,(g)H,O(g)102-948136-1131214-394189-242AHxn = [ ? ] kJ%3DEnter either a + or - sign AND the magnitude.Enthalpy (kJ)Enter

In this question we have to tell the change in enthalpy of the given reaction.

Using the data below, calculate the enthalpy for the decomposition of sodium bicarbonate. 2NaHCO3(s) NażCO3(s) + H2O(g) + CO2(g) Compounds S (/mol-K) AHf° (kJ/mol) NaHCO,(s) Na,Co,(s) Co,(g) H,O(g) 102 -948 136 -1131 214 -394 189 -242 AHxn = [ ? ] kJ %3D Enter either a + or - sign AND the magnitude.

Using the data below, calculate the enthalpy for the decomposition of sodium bicarbonate. 2NaHCO3(s) NażCO3(s) + H2O(g) + CO2(g) Compounds S (/mol-K) AHf° (kJ/mol) NaHCO,(s) Na,Co,(s) Co,(g) H,O(g) 102 -948 136 -1131 214 -394 189 -242 AHxn = [ ? ] kJ %3D Enter either a + or - sign AND the magnitude.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.79E: The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C...

See similar textbooks

Similar questions

Gasohol, a mixture of gasoline and ethanol, C2H5OH, is used as automobile fuel. The alcohol releases energy in a combustion reaction with O2. C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) If 0.115 g ethanol evolves 3.62 kJ when burned at constant pressure, calculate the combustion enthalpy for ethanol.
In a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed to yield the following reaction: Ag+(aq)+Cl(aq)AgCl(s) The two solutions were initially at 22.60C, and the final temperature is 23.40C Calculate the heat that accompanies this reaction in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 100.0 g and a specific heat capacity of 4.18J/Cg.
9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?
The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.
White phosphorus, P4, ignites in air to produce P4O10. When 3.56 g P4 is burned, 85.8 kJ of thermal energy is evolved at constant pressure. Calculate the combustion enthalpy of P4.
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?
In a constant-volume calorimeter, 35.0g of H2cools from 75.3C to25.0C. Calculate w, q, U, and H for the process.
Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
Nitrogen gas (2.75 L) is confined in a cylinder under constant atmospheric pressure (1.01 105 pascals). The volume of gas decreases to 2.10 L when 485 J of energy is transferred as heat to the surroundings. What is the change in internal energy of the gas?
In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCI is added to 50.0 mL of 1.00 M NaOH to make 200.0 g solution at an initial temperature of 48.2C. If the enthalpy of neutralization for the reaction between a strong acid and a strong base is 56 kJ/mol, calculate the final temperature of the calorimeter contents. Assume the specific heat capacity of the solution is 4.184 J/g C and assume no heat Joss to the surroundings.