The equilibrium between NO2 and N2O4 can be described by the following equation:

2NO2(g) ⇌ N2O4(g) Kp = 7.0

If a sealed flask contains 1.5 atm of NO2 and 14.2 atm of N2O4. Calculate the value of Kc for the reaction,

The question is incomplete, here is the complete question:

The equilibrium between NO₂ and N₂O₄ can be described by the following equation:

2NO₂(g) ⇌ N₂O₄(g); Kp = 7.0

If a sealed flask contains 1.5 atm of NO₂ and 14.2 atm of N₂O₄. Calculate the value of Kc for the reaction at 25°C

The value of for given reaction is 171.3

Explanation:

For the given chemical equation:

Relation of is given by the formula:

Where,

= equilibrium constant in terms of partial pressure = 7.0

= equilibrium constant in terms of concentration

R = Gas constant =

T = temperature =

= change in number of moles of gas particles =

Putting values in above equation, we get:

Hence, the value of for given reaction is 171.3

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.