For the answer to the questions above,
a) Ag2CO3(s) => Ag2O(s)+CO2(g)
<span>b) Cl2(g)+2(KI)(aq) => I2(s)+2(KCl)(aq) (coefficients are for balanced equation) </span>
<span>net ionic is Cl2(g)+2I- => I2(s)+2Cl-(aq) </span>
<span>c) I2(s)+3(Cl2)(g)=>2(ICl3)
</span>I hope I helped you with your problem
At 218 °C, solid NH₄SH decomposes to form 0.011 M NH₃ and H₂S, as given by its equilibrium constant.
<h3>What is the equilibrium constant?</h3>
The equilibrium constant (Keq) is the ratio of the product of the concentrations of the products to the product of the concentrations of the reactants, all raised to their stoichiometric coefficients.
Only gases and aqueous species are included.
- Step 1. Make an ICE chart.
NH₄SH(s) ⇋ NH₃(g) + H₂S(g)
I 0 0
C +x +x
E x x
- Step 2. Write the equilibrium constant.
Keq = 1.2 × 10⁻⁴ = [NH₃] [H₂S] = x²
x = 0.011 M
At 218 °C, solid NH₄SH decomposes to form 0.011 M NH₃ and H₂S, as given by its equilibrium constant.
Learn more about equilibrium here: brainly.com/question/5081082
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I think the answer is that three electrons are gained, creating N-3
Answer:
mol·L⁻¹·s⁻¹
Explanation:
In the case of a <em>zero-order reaction</em>, the reaction rate does not change with the decrease or increase in the concentrations of the reactants:
And because the rate must have units of mol·L⁻¹·s⁻¹, then the rate constant <em>k</em> must also have units of mol·L⁻¹·s⁻¹.
