Answer:
See explanation
Explanation:
The reaction to be considered is shown below;
H2CO3<------->CO2 + H2O
We know that when a constraint such as a sudden change in concentration, pressure or temperature is imposed on a reaction system in equilibrium, the system has to adjust itself by shifting in a particular direction in order to cancel the constraint.
Now, if we remove CO2, the equilibrium position must shift to the right by the decomposition of more H2CO3 to establish equilibrium again.
Q = mcΔθ
67.5 = m x 0.45 x (28.5 - 21.5)
M = 67.5 / 3.15
= 21.4 g
The reaction between copper II chloride and sodium sulfide as well as lead II nitrate and potassium sulfate both produce precipitates.
The solubility of a substance in water is in accordance with the solubility rules. It is possible that a solid product may be formed when two aqueous solutions are mixed together. That solid product is referred to as a precipitate.
Now, we will consider each reaction individually to decode whether or not a precipitate is possible.
- In the first reaction, we have; CuCl2(aq) + Na2S(aq) ---->CuS(s) + 2NaCl(aq). A precipitate (CuS) is formed.
- In the second reaction, Pb(NO3)2(aq) + 2KNO3(aq) ----> PbSO4(s) + KNO3(aq), a precipitate PbSO4 is formed
- In the third reaction, NH4Br(aq) + NaOH(aq) ----->NH3(g) + NaBr(aq) + H2O(l), a precipitate is not formed here.
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