Chemistry, 21.11.2019 09:31 nicog94

The reaction between hydrogen and oxygen to yield water vapor has δh∘=−484kj: 2h2(g)+o2(g)→2h2o(g)δh∘=−484kj

how much pv work is done in kilojoules for the reaction of 3.20 mol of h2 with 1.60 mol of o2 at atmospheric pressure if the volume change is −22.6l?

express your answer using three significant figures

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Answer from: fordd4

The PV work in kilojoules for the reaction is $\boxed{2.29\;{\text{kJ}}}$ .

Further Explanation:

First law of thermodynamics:

The law states that energy cannot be created or destroyed but only changes its form and versa.

The internal energy of the system defines the total energy of the system and is sum of enthalpy of the system and work done. Internal energy only depends on the temperature of the system. The mathematical expression of the internal energy is as follows:

${\text{U}} = {\text{H}} + {\text{W}}$

Where,

U is the internal energy of the system.

H is the enthalpy of the system.

W is the work-done.

The formula for workdone by the system is as follows:

${\text{W}} = - {\text{P}}\Delta {\text{V}}$

Where,

P is the pressure in atmosphere.

$\Delta {\text{V}}$ is the change in the volume in liter.

The atmospheric pressure is $1\;{\text{atm}}$ .

The change in volume is $- 22.6\;{\text{L}}$ .

Substitute these values in above equation to calculate the work done by the system.

$\begin{aligned}{\text{W}}&= - {\text{P}}\Delta {\text{V}}\\&= - \left( {1\;{\text{atm}}} \right)\left( { - 22.6\;{\text{L}}} \right)\\&= 22.6\;{\text{L}} \cdot {\text{atm}}\left( {\frac{{0.101325\;{\text{kJ}}}}{{1\;{\text{L}} \cdot {\text{atm}}}}} \right)\\&= 2.2899\;{\text{kJ}}\\\end{aligned}$

The correct answer in 3 significant figures is $2.29\;{\text{kJ}}$ .

Learn More:

Determine the enthalpy of a reversed reaction: Find the enthalpy change of a reaction:

Answer Details:

Grade: Senior School

Chapter: Thermodynamics

Subject: Chemistry

Keywords: Internal energy,thermodynamics,PV work, kilojoules, volume change, enthalpy, work done. significant figures,2.29KJ, atmospheric pressure.

Answer from: Quest

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

Answer from: Quest

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

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The reaction between hydrogen and oxygen to yield water vapor has δh∘=−484kj: 2h2(g)+o2(g)→2h2o(g)δ...

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