Please help me on this question I'm confusied on it
2 answers:
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Answer:
Kc for this equilibrium is 2.30*10⁻⁶
Explanation:
Equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction and the concentrations of reactants and products are held constant.
Being:
aA + bB ⇔ cC + dD
the equilibrium constant Kc is defined as:
In other words, the constant Kc is equal to the multiplication of the concentrations of the products raised to their stoichiometric coefficients by the multiplication of the concentrations of the reactants also raised to their stoichiometric coefficients. Kc is constant for a given temperature, that is to say that as the reaction temperature varies, its value varies.
In this case, being:
2 NH₃(g) ⇔ N₂(g) + 3 H₂(g)
the equilibrium constant Kc is:
Being:
- [N₂]= 0.0551 M
- [H₂]= 0.0183 M
- [NH₃]= 0.383 M
and replacing:
you get:
Kc= 2.30*10⁻⁶
<u><em>Kc for this equilibrium is 2.30*10⁻⁶</em></u>
<u>Answer:</u> The amount of barium sulfate produced in the given reaction is 0.667 grams.
<u>Explanation:</u>
To calculate the number of moles from molarity, we use the equation:
Molarity of barium chloride = 0.113 M
Volume of barium chloride = 25.34 mL = 0.02534 L (Conversion factor: 1 L = 1000 mL)
Putting values in above equation, we get:
For the given chemical reaction:
By Stoichiometry of the reaction:
1 mole of barium chloride is producing 1 mole of barium sulfate.
So, 0.00286 moles of barium chloride will produce = of barium sulfate.
Now, to calculate the mass of barium sulfate, we use the equation:
Molar mass of barium sulfate = 233.38 g/mol
Moles of barium sulfate = 0.00286 moles
Putting values in above equation, we get:
Hence, the amount of barium sulfate produced in the given reaction is 0.667 grams