Table of Contents

## What is the enthalpy of H2SO4?

Enthalpy of formation of gas at standard conditions (nominally 298.15 K, 1 atm.)

ΔfH°gas (kJ/mol) | -735.13 |

Method | Review |

Reference | Chase, 1998 |

Comment | |
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Data last reviewed in September, 1977 |

## What is the enthalpy of neutralization of NaOH and H2SO4?

neutralisation is more exactly H+ from acid reacting with OH- of alkali. this is according to the stoichiometric equation. when you react 0.5 mol H2SO4 with 1 mol NaOH, you get -57 kJmol-1. if you use 1 mol H2SO4 with 2 mol NaOH you will get about -114 kJmol-1.

## What is the enthalpy of neutralization for HCl and NaOH?

Enthalpy of Neutralization: Strong Diprotic Acid and Strong Monobasic Base

HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) | ΔHneut = -55.2 kJ mol-1 (of water) |
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H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l) | ΔHneut = -55.8 kJ mol-1 (of water) |

## What is the molar enthalpy of neutralization for sulfuric acid?

The enthalpy of neutralization of H2SO4 is in fact the enthalpy of water formation: H2SO4 + 2NaOH → Na2SO4 + 2H2O; OH- + H+ → H2O; Thus, the molar enthalpy for this reaction is -57.62 kJ/mol at 25 C.

## How do you calculate enthalpy of dilution?

Therefore, the molar integral enthalpy of dilution (also known as the molar integral heat of dilution) can be evaluated by calculating the total enthalpy change associated with the change in the dilution of the solution (from its initial concentration to its final concentration) and normalizing this value by the number …

## How do you calculate enthalpy of neutralization?

Calculate the heat of neutralization using the fomula Q = mcΔT, where “Q” is the heat of neutralization, “m” is the mass of your acid, “c” is the specific heat capacity for aqueous solutions, 4.1814 Joules(grams x °C), and “ΔT” is the change in temperature you measured using your calorimeter.

## Is enthalpy of neutralization always negative?

Enthalpy changes of neutralization are always negative – heat is released when an acid and and alkali react. For reactions involving strong acids and alkalis, the values are always very closely similar, with values between -57 and -58 kJ mol-1.

## How is enthalpy of neutralization calculated?

Calculate the number of moles of base you add to determine the molar heat of neutralization, expressed using the equation ΔH = Q ÷ n, where “n” is the number of moles. For example, suppose you add 25 mL of 1.0 M NaOH to your HCl to produce a heat of neutralization of 447.78 Joules.

## What is the enthalpy of dilution example?

The heat of a solution of NaOH in water, the heat of solution of 1.0 mole of NaOH in 5 moles of water and in 200 moles of water are respectively – 37.8 and -42.3 kJ. Thus, in the above example of enthalpy of solution of NaOH the difference between the two values, – 4.5 kJ would be the enthalpy of dilution.