At -10.8 °C the concentration equilibrium constant Kc = 4.0 x 10^-5 . for a certain reaction Here are some facts about the reaction:

If the reaction is run at constant pressure, the volume increases by 14.9% .
The constant pressure molar heat capacity Cp= 2.63 J-mol^-1. K^-1.
If the reaction is run at constant pressure, 120. kJ/mol of heat are released.

Using these facts, can you calculate Kc at -16.°C?

K2 = 9.701 x 10^-10

Explanation:

K1 = 4.0 x 10^-5

K2 = ?

T1 = -10.8 °C +273 = 262.2K

T2 =  -16 °C + 273 = 257K

ΔHrxn = 120. kJ/mol = 120000 J/mol

The formular relating all these parameters is given as;

ln( K2 / K1)  =  −ΔHrxn / R  * (1 / T2 − 1 / T1)

ln (K2 / 4.0 x 10^-5) = - 120000 / 8.314 (1 / 257 - 1 / 262.2)

ln (K2 / 4.0 x 10^-5) = 1.1138

ln K2 - ln4.0 x 10^-5 = 1.1138

ln K2 = 1.1138 + ln4.0 x 10^-5

ln K2 = 1.1138 - 10.1266

ln K2 = -9.0128

K2 = 9.701 x 10^-10

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

a boiling water reactor does not boil the water. a pressurized water reactor boils the water faster. a pressurized water reactor is heated directly by the core. a pressurized water reactor does not use fission.