Consider the following system at equilibrium:
N2(g)+3H2(g)-2NH3(g)

What will happen to this system if 1.00 mol N subscript 2 is suddenly added?

Group of answer choices

The additional collisions between N subscript 2 and H subscript 2 molecules increases the rate in the forward direction and produces more N H subscript 3

The concentrations of each molecule would increase relative to the original amount present.

As the concentration of N H subscript 3 increases, equilibrium shifts to the left and increases H subscript 2 concentration.

The sudden change in the amount of N subscript 2 increases the rate in the reverse direction to compensate and produce more H subscript 2.

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.

the correct answer to this question is 2