Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2no2 → 2no + o2 in a particular experiment at 300 °c, [no 2 ] drops from 0.0100 to 0.00650 m in 100 s. the rate of disappearance of no2 for this period is m/s.

The rate of disappearance of is

Explanation:

The given chemical reaction is:

The rate of the reaction for disappearance of is given as:

Or,

where,

= final concentration of = 0.00650 M

= initial concentration of = 0.0100 M

= final time = 100 minutes

= initial time = 0 minutes

Putting values in above equation, we get:

Hence, the rate of disappearance of is

how about u try it first

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm