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Marianna [84]
3 years ago
12

The enthalpy change, ΔH, for a reaction at constant pressure is defined as: ΔH = ΔE + PΔV. For which of the following reactions

will ΔH be approximately equal to ΔE? Select all that apply. Group of answer choices 2 NO2(g) -> N2(g) + 2 O2(g)
Chemistry
1 answer:
OleMash [197]3 years ago
5 0

The given question is incomplete. The complete question is:

The enthalpy change, ΔH, for a reaction at constant pressure is defined as: ΔH = ΔE + PΔV. For which of the following reactions will ΔH be approximately equal to ΔE? Select all that apply. Group of answer choices

2NO_2(g)\rightarrow N_2(g)+2O_2(g)

Ca(OH)_2(aq)+H_2SO_4(aq)\rightarrow 2H_2O(l)+caSO_4(s)

C(s)+O_2(g)\rightarrow CO_2(g)

None of the above

Answer:  

C(s)+O_2(g)\rightarrow CO_2(g)

Explanation:

Relation of  with  is given by the formula:

\Delta H=\Delta E+{\Delta n_g}RT     as

Where,

\Delta H = enthalpy change

\Delta E= internal energy change

R = Gas constant

T = temperature

\Delta n_g= change in number of moles of gas particles = n_{products}-n_{reactants}

1. For 2NO_2(g)\rightarrow N_2(g)+2O_2(g)

\Delta n_g=n_{products}-n_{reactants}=(3-2)=1

2. For Ca(OH)_2(aq0+H_2SO_4(aq)\rightarrow 2H_2O(l)+CaSO_4(s)

\Delta n_g=n_{products}-n_{reactants}=(0-0)=0

3.  C(s)+O_2(g)\rightarrow CO_2(g)

\Delta n_g=n_{products}-n_{reactants}=(0-0)=0

Thus for reactions 2 and 3,  ΔH be approximately equal to ΔE

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