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.
1 answer:
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
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
an exothermic reaction
as endothermic or exothermic
an exothermic dissolving process
Keywords: exothermic, endothermic, enthalpy, internal energy, heat
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