Hydrogen fuel cells are a promising alternative to gasoline engines in part because they release water instead of carbon dioxide
2 answers:
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Answer:
see below
Explanation:
Aqueous hydroiodic acid reacts with liquid water in a reversible reaction.
2 HI + 2 H₂O ⇔ 2 H₃O + I₂
This is an acid-base reaction. HI is the acid, and H₂O is the base. The conjugate acid is H₃O, and the conjugate base is I₂. You can figure out the acid and base by a using a table of strong/weak acids and bases. The conjugate will have one less or one more H⁺ depending on if it's an acid or a base.
The expression for Kₐ of the reaction is below. You have to put the acid and its conjugate base on the top and the base and its conjugate on the bottom. I didn't put in H₂O since, although it is the base in this equation, it isn't really a base.
Solid zinc reacts with solid manganese (IV) oxide producing solid zinc oxide and solid manganese (III) oxide.
Zn + 2 MnO₂ ⇒ ZnO + Mn₂O₃
This is a redox reaction. The Zn is being oxidized, and the Mn is being reduced.
Oxidation: Zn ⇒ Zn⁺² + 2 e⁻
Reduction: Mn⁺⁴ + e⁻ ⇒ Mn⁺³
Aqueous silver nitrate reacts with aqueous calcium chloride.
2 AgNO₃ + CaCl₂ ⇒ 2 AgCl + Ca(NO₃)₂
This is a precipitation reaction. You have two soluble salts combing to form a solution. You now need to figure out which of the compounds produced are not soluble. AgCl is the compound that is not soluble in water, making it the precipitate.
I think I covered everything. If I missed something let me know.
The full question can be seen below:
The decomposition of is represented by the equation above.
A student monitored the decomposition of a 1.0 L sample of at a constant temperature of 300K and recorded the concentration of
as function of time. The results are given in the table below:
Time (s)
0 2.7
200 2.1
400 1.7
600 1.4
The produced from the decomposition of the 1.0 L sample of
is collected in a previously evacuated 10.0 L flask at 300 K. What is the approximate pressure in the flask after 400 s?
(For estimation purpose, assume that 1.0 mole of gas in 1.0 L exerts a pressure of 24 atm at 300 K).
Answer:
1.2 atm
Explanation:
Considering all assumptions as stated above;
Initial 2.7 mole --- ---
Change -1.0 ---
Equilibrium 1.7 mole --- 0.5 mole
To determine the concentration of O₂; we need to convert the moles to concentration for O₂ =
=
= 0.05
Thus, based on the assumption that "1.0 mole of gas in 1.0 L exerts a pressure of 24 atm"
∴ 0.05 will give rise to = 0.05
× 24
= 1.2 atm