Answer:
Explanation:
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In this case, in agreement to the given chemical reaction, it is possible for us to calculate the mass of NH3 required to remove 57.0 g NO via the stoichiometry based off the 4:6 mole ratio between them:
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Answer:
Different types
Explanation:
Because it's in a different place
Δ H reaction = q / n where q: amount of heat released and n is number of moles of substance.
q = m . C . ΔT where:
m = mass of substance (g)
C = Specific heat capacity (4.18)
ΔT = change in temperature = 24.25 - 23.16 = 1.09
q = 1000 x 4.18 x 1.09 = 4556 J = 4.556 kJ
number of moles (n) = Molarity (M) x Volume (L)
= 0.185 M x 0.07 L = 0.01295 mole
Δ H = q / n = - (4.556 kJ / 0.01295 mole) = -351.8 kJ / mol
Note: it is exothermic reaction (-ve sign) i.e. temperature is raised
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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Answer:
Carbon
Explanation:
I just finished this and that's what I got from my periodic table.
