The decomposition of sulfuryl chloride into sulfur dioxide and chlorine SO2Cl2(g) → SO2(g) + Cl2(g) follows first-order kinetics. At 320◦C the rate constant is 2.2 × 10−5 sec−1 . If one started with a sample containing 0.16 moles of sulfuryl chloride per liter at 320◦C, what concentration would be left after 6.00 hours?

The concentration of sulfuryl chloride left is 0.0995 M

Explanation:

For the given chemical equation:

Rate law expression for first order kinetics is given by the equation:

where,

k = rate constant  =

t = time taken for decay process = 6.00 hours = (6 × 3600) = 21600 s    (Conversion factor:  1 hr = 3600 seconds)

= initial amount of the sample = 0.16 moles

[A] = amount left after decay process =  ?

Putting values in above equation, we get:

Molarity is calculated by using the equation:

Moles of sulfuryl chloride left = 0.0995 moles

Volume of solution = 1 L

Hence, the concentration of sulfuryl chloride left is 0.0995 M

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation:

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.