Consider 1 mol of a gas initially at 273 K and 1.00 atm in a 10.0 L vessel. i) I

Question

Consider 1 mol of a gas initially at 273 K and 1.00 atm in a 10.0 L vessel. i) If the volume of the container is reduced to 5.0 L, will the pressure increase or decrease? Justify your answer using kinetic molecular theory. ii) If the temperature in the vessel is reduced to 185 K. will the pressure increase or decrease? Justify your answer using kinetic molecular theory. The Haber process is the principal method for converting nitrogen into ammonia. N_2(g) + 3H_2 (g)right arrow 2 NH^3 (g) What volume of NH_3 (g) can be produced from 152 L of N_2(g) and 313 L of H:(g) if the gases are measured at 315degreeC and 5.25 atm.

Explanation / Answer

a)

if volume reduces, then the pressure increases (boyle law)

P1V1 = P2V2

there are more molecules per unit space, therefore the crash more often to th econtainer wall

aii)

IF T is reduced, then th epressure must decrease, since less collision of polecules will exist

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