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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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Determine the limiting reactant (lr) and the mass (in g) of nitrogen that can be formed from 50.0 g n2o4 and 45.0 g n2h4. some p
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1) to calculate the limiting reactant you need to pass grams to moles.
<span> moles is calculated by dividing mass by molar mass
</span>
mass of N2O4: 50.0 g 
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</span><span>molar mass of N2H4 = 32.05 g/mol.
</span>mass of N2H4:45.0 g

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</span> 2)</span>
By looking at the balanced equation, you can see that 1 mol of N2O4 needs 2 moles of N2H4 to fully react . So to react  0,54 moles of N2O4, you need 2x0,54 moles of <span>N2H4 moles
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3) 1 mol of N2O4 reacting, will produce 3 mol of N2 (look at the equation)
There are 0,54 mol of N2O4 available to react, so how many moles will produce of N2?
1 mol N2O4------------3 mol of N2
0,54 mol N2O4--------x
x=1,62 mol of N2

4) the only thing left to do is convert the moles obtained, to grams.
We use the same formula as before, moles equal to mass divided by molar mass.
moles= \frac{grams}{molar mass}             (molar mass of N2= 28)
1,62 mol of N2= mass/ 28
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Zielflug [23.3K]
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