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6. A student dissolved 1.1 g of solid NaOH in 22.1 mL of water inside a constant-pressure
calorimeter. As the reaction solution is mixed, temperature of the solution increases
from 18.2 °C to 31.4 °C. Calculate the AH for the dissolution of NaOH in kJ/mol as
measured by the student.
Assume that he specific heat of the solution is same as that of water (4.184 J/g. °C) and
the density of solutions is same as that of water (1.00 g/mL)

6 A student dissolved 11 g of solid NaOH in 221 mL of water inside a constantpressure calorimeter As the reaction solution is mixed temperature of the solution class=

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From the calculations, the heat of the reaction is 44.4 kJ/mol.

What is the enthalpy of reaction?

The enthalpy of reaction refers to the amount of heat that is absorbed or evolved in a reaction.

Number of moles of NaOH = 1.1 g /40 g/mol = 0.0275 moles

Mass of the water = 22.1 mL or 22.1 g

Given that;

H= mcdT

H = 22.1 g *4.184 * (31.4 - 18.2)

H = 1221 J or 1.221kJ

ΔH rxn = -(1.221kJ)/0.0275 moles

ΔH rxn = 44.4 kJ/mol

Learn more about enthalpy:https://brainly.com/question/15319033

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