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RSB [31]
2 years ago
15

A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the v

olume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules.

Chemistry
1 answer:
Eduardwww [97]2 years ago
4 0

The value of the total energy change, ΔE, in kilojoules = -61.93 kJ

<h3>Further explanation</h3>

Thermochemistry is a branch of chemistry that studies heat changes in chemical reactions.

Thermochemistry is the application of thermodynamics to chemistry.

Thermochemistry is used to predict energy changes in:

  • 1. chemical reaction
  • 2. change in form
  • 3. solution

Energy in (E) is the energy contained in a material

Internal energy is affected by heat changes and work (w)

Delta H reaction (ΔH) is the amount of heat change between the system and its environment

(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)

Enthalpy (H) is a state function which is the sum of the Energy in (E) and work (w).

At constant pressure (P = fixed), the change in entalphy can be formulated:

ΔH = ΔE + P. ΔV

\large{\boxed{\bold{\Delta E=\Delta H-P.\Delta V}}}

From the problem it can be seen that

ΔH = -75.0 kJ

Pressure, P = 43.0 atm

= 43 atm x 1,01325 .10⁵ Pa / atm

= 4,357.10⁶ Pa

= 4,357.10⁶ N / m²

Volume changes that occur

ΔV = 2.0 L - 5.0 L

= -3.0 L

= -3.0 x 10⁻³ m³

= 1.3071.10⁴ J

= 13,071 kJ

So that:

ΔE = ΔH - PΔV

ΔE = -75.0 kJ - (4,357.10⁶ .- 3.0 x 10⁻³ m3)

ΔE = -75.0 kJ + 13,071 kJ

ΔE = -61.93 kJ

<h3>Learn more</h3>

Delta H solution

brainly.com/question/10600048

an exothermic reaction

brainly.com/question/1831525

 as endothermic or exothermic

brainly.com/question/11419458

an exothermic dissolving process

brainly.com/question/10541336

Keywords: exothermic, endothermic, enthalpy, internal energy, heat

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<u>Answer:</u>

<u>For a:</u> The mass of acetic anhydride needed is 73.91 grams.

<u>For b:</u> The theoretical yield of aspirin is 130.43 grams.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}   .....(1)

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Putting values in equation 1, we get:

\text{Moles of salicylic acid}=\frac{100g}{138.121g/mol}=0.724mol

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By stoichiometry of the reaction:

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So, 0.724 moles of salicylic acid will react with = \frac{1}{1}\times 0.724=0.724mol of acetic anhydride.

Now, to calculate the mass of acetic anhydride, we use equation 1:

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Putting values in equation 1, we get:

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  • <u>For b:</u>

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So, 0.724 moles of salicylic acid will produce = \frac{1}{1}\times 0.724=0.724mol of aspirin.

Now, to calculate the mass of aspirin, we use equation 1:

Moles of aspirin = 0.724 moles

Molar mass of aspirin = 180.158 g/mol

Putting values in equation 1, we get:

0.724mol=\frac{\text{Mass of aspirin}}{180.158g/mol}\\\\\text{Mass of aspirin}=130.43g

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