Answer:
A. To focus on only those ions that form the precipitate
Explanation:
Net ionic equations cancel out the ions that appear on both sides of the reaction because they essentially don't participate in the reaction. This is very useful when dealing with redox reactions because are complicated enough without spectator ions being in the way, so they help focus on those ions that actually form the precipitate.
Key Terms
- Spectator Ions: an ion that does not take part in the chemical reaction.
- Net ionic equations: a equation where ions that appear on both sides are canceled out.
- Redox reaction: an oxidation-reduction reaction.
TTTTTTTTTTTTNSNSKDKDLDDHKD
Answer:
Hydrated chromium(III) phosphate or chromium(III) phosphate tetrahydrate.
Answer:
K = [H2] [CO] / [HCHO]
Explanation:
HCHO(g) ⇌ H2(g) + CO(g)
We can obtain the expression for the equilibrium constant for the above equation as follow:
Equilibrium constant, K for a given reaction is the ratio of the concentration of the product raised to their coefficient to the concentration of the reactant raised to their coefficient.
Thus, the equilibrium constant, K for the above equation can be written as follow:
K = [H2] [CO] / [HCHO]
