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23 cze 2023 · Solution. According to Le Chatelier's principle, if pressure is increased, then the equilibrium shifts to the side with the fewer number of moles of gas. This particular reaction shows a total of 4 mol of gas as reactants and 2 mol of gas as products, so the reaction shifts toward the products side.
30 sty 2023 · In a hypothetical reaction: aA (s) + bB (l) ⇌ gG (aq) + hH (aq) The equilibrium constant expression is written as follows: Kc = [G]g[H]h 1 × 1 = [G]g[H]h. In this case, since solids and liquids have a fixed value of 1, the numerical value of the expression is independent of the amounts of A and B.
15 maj 2013 · You have the reaction $$\ce{H2(g) + O2(g) <=> H2O2(g)}$$ at $T = 500\ \mathrm{K}$. The reaction reaches equilibrium at the following concentrations: $$\ce{[H2]} = \ce{[O2]} = 5 \times 10^{-3}\ \mathrm{mol\ dm^{-3}}$$ $$\ce{[H2O2]} = 4\times10^{-5}\ \mathrm{mol\ dm^{-3}}$$ This gives $$K_c = \left(\frac{\ce{[H2O2]}}{\ce{[H2][O2]}}\right) = 1.6$$
13 maj 2023 · The equilibrium constant for the decomposition of CaCO3 (s) to CaO (s) and CO2 (g) is K = [CO2]. At 800°C, the concentration of CO2 in equilibrium with solid CaCO3 and CaO is 2.5 × 10 − 3 M. Thus K at 800°C is 2.5 × 10 − 3 (remember that equilibrium constants are unitless).
The principle that you need to rely on to find a proper base is that any acid-base reaction lies to the side of forming a weaker acid and a base. Remember, a strong acid and a base react to form a weak acid and a base.
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