Anyone good in chemistry im stumped!?

Question

Considering the reaction: N2(g) + 3H2(g) → 2NH3(g)

Explain why this reaction is spontaneous even though it results in matter being less dispersed

Answer 1

The first answer is correct.

The second answer confuses kinetics with thermodynamics. A catalyst only affects the rate of the reaction and has no bearing on the spontaneity of the reaction. A catalyst is used in the Haber process to reduce the amount of residence time needed in the reactor.

Answer 2

Even though the entropy decreases, the enthalpy is negative enough to make the reaction spontaneous. The formula is DeltaG=DeltaH-(T)DeltaS
G is the free energy
T is the temperature
S is the entropy

if DeltaG is negative, then the reaction is spontaneos.
since DeltaS is negative, the -TDeltaS term is positive
this positive term is trying to make the reaction nonspontaneous
if the reaction is in fact spontaneous, then the DeltaH(enthalpy) must be low enough to offset the positive TDeltaS.

Thus the enthalpy is just very negative

Answer 3

Parts per million (ppm) is as the name suggests, 1 part of mass, volume, etc, dissolved in 1,000,000 parts of mass, volume, etc. Relation of units of mass / volume must be in a proportion of 1,000,000 one respect the other: For example, mg/L obey this rule, g/metric ton obey this rule, mg/Kg, mL/m³, etc obey this rule. In your example, 0.0700 grams of arsenic in 10 Liters of water, you just have to convert the grames to miligrames: 0.07 grams x1000 = 70 miligrams So you just apply: 70 mg/10 L = 7 mg/L = 7 ppm Hope it was clear! Good luck!

Answer 4

Hydrogen is a reactive material. In the compoundammonia i is more stable