Given the following information: aHCO3(s)+85 kJ Na2CO3(s)+H2O(1) CO2(g) Calculate the amount of heat (ink) required to decompose 2.24 mol NaHCO3(s). You must show your work to receive credit .

The amount of heat required comes out to be 190.4 KJ

Explanation:

The reaction for the decomposition of is shown below

Amount of heat required to decompose 1 mole  = 85 KJ

Amount of heat required to decompose 2.24 mole =

Amount of heat required = 190.4 KJ

did anyone actually do this? like if anyone has submitted this i rly need .

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