A flask of volume 5.00 L is evacuated and 43.78 g of solid dinitrogen tetroxide, N2O4, is introduced at ?196°C. The sample is then warmed to 25°C, during which time the N2O4 vaporizes and some of it dissociates to form brown NO2 gas. The pressure slowly increases until it stabilizes at 2.96 atm. (a) Write a balanced equation for the reaction. (b) If the gas in the flask at 25°C were all N2O4, what would the pressure be? (c) If all the gas in the flask converted into NO2, wha

help me.

Explanation:

jkqn cn c

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml