Answer:
See the answer below, please.
Explanation:
The equilibrium constant is defined as the relationship between products and reagents, each one elevated to their stoichiometric coefficients, in that of the given equation, the Kc is:
Kc= (NH4)^1/ (NH3)^1 x (HI)^1
NH4= products
NH3 and HI = reagents
You must know and use the formula for pH.
pH = - log [H3O+], where [H3O+] is the molar concentration of hydronium ion.
So, when pH is 8.0 => 8.0 = - log [H3O+] and you can use antilogarithm (the inverse function of logarithm) to find [H3O+], in this way:
[H3O+] = 10^-8 = 1 * 10 ^-8 M
When, pH = 7.0 =>
7.0 = - log [H3O+] => [H3O+] = 1 * 10^ -7 M
Answer: 1*10^-7 mole / liter
An exergonic reaction proceeds with net release of free energy.
An endergonic reaction absorbs free energy
Answer:
Mg S2 O3
Explanation:
.691 g of Mg is .284 mole
1.84 g of S is .5739 mole
1.365 g of O is .8531 mole you can see the ratio is ~ 1 :2 :3
Mg S2 O3
