`N_(2)O_(5(g))` is at a pressure of 0.5 atm. After 100 s the pressure of the decomposition mixture is 0.512 atm. Calculate the rate constant.

Thermal decomposition for N_2O_5(g) follows 1st order kinetics as per N_2O_5(g) to 2NO_2(g) + 1/2O_2(g) . Initial pressure of N_2O_5 is 100mm. After 10 minutes, the pressure developed is 130mm, what is rate constant?

In a mixture of N_2 and CO_2 gases, the partial pressure of CO_(2) is 1.25 atm. The total pressure of the mixture is 5 atm. The mole fraction of N_(2) in the mixture is

A vessel at 100K contains CO_(2) with a pressure of 0.5 atm. Some of the CO_(2) is converted into CO on addition of graphite. Calculate the value of K if total pressure at equilibrium is 0.8 atm.

100 mL of 1.5% (w/v) solution of urea is found to have an osmotic pressure of 6.0 atm and 100 mL of 3.42% (w/v) solution of cane sugar is found to have an osmotic pressure of 2.4 atm. If the two solution are mixed the osmotic pressure of the resulting solution in atm is Assume that there is no reaction between urea and cane sugar )

The temperature of 5 moles of a gas is decreased by 2K at constant pressure of 1 atm. Indicate the correct statement

A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What is K_(p) for the given equilibrium ? 2HI(g)hArrH_(2)(g)+I_(2)(g)

In a closed container NO_(2) gas is getting dimerised into N_(2)O_(4) gas with first order kinetics. Pressure after 10 hours of reaction is 5 atm and pressure after completion of reaction is 4atm. What is half life in hours?