Which equation is associated with the third ionization energy of aluminum?
Al2+(g) → Al3+(g) + e- |
||
Al(g) + 3e- → Al3-(g) |
||
Al(g) → Al3+(g) + 3e- |
||
Al3+(g) → Al(g) + 3e- |
Answer -
We know that,
Ionization energy is the energy needed to remove one mole electrons from one mole of atoms in the gaseous state. i.e.
X (g) + energy X+ (g) + e-
So, For Aluminum,
Al (g) + 1st Ionization Energy Al+ (g) + e-
Al+ (g) + 2nd Ionization Energy Al2+ (g) + e-
Al2+ (g) + 3rd Ionization Energy Al3+ (g) + e-
So, Al2+(g) → Al3+(g) + e- [ANSWER]
Which equation is associated with the third ionization energy of aluminum? Al2+(g) → Al3+(g) + e-...
Which of the following is the reaction associated with the first ionization energy of nitrogen? A) N(g) → N+ + e- B) N(g) → N3+ + 3e- C) N(g) + 3e- → N3- D) N(g) → N- + e- E) N(g) + e- → N- chemistry
For which of the following reactions is the enthalpy change equal to the third ionization energy of vanadium? O v3+(g) - V4*(g) +- O v2(g) → V3+(g) + O v3*(g) +e*V2+(g) O v2-19) +eV3–(9) O vig) -V3+(g) + 3e
Which of the statements listed below is false? a) The third ionization energy of Al is greater than the third ionization energy of Mg. b) The second ionization energy of Na is greater than the second ionization energy of Mg. c) The first ionization energy of Be is greater than the first ionization energy of Li. d) The first ionization energy of Li is greater than the first ionization energy of Na. e) The fourth ionization energy of C is...
Write a chemical equation representing the third ionization energy for lithium. Use e as the symbol for an electron. chemical equation:
12. Which of the following correctly represents the second ionization of aluminum? A) Ait (g) + € → Al (9) B) AI (g) → Al* (g) + e C) Al-(g) + e + A1-(g) D) A1+ (g) + e* → A12+ (8) E) A1+ (g) → A12+ (g) + e*
Which one of the following chemical equations refers to the second ionization of Al? A) Al(s) + 2e– –––> Al2–(s) B) Al+(g) –––> Al2+(g) + e– C) Al(g) –––> Al2+(g) + 2e– D) Al(s) –––> Al+(s) + e– E) Al2+(g) + e– –––> Al+(g)
Determine the mass (g) of aluminum deposited in an electrolytic cell using a current of 0.750 A for 1.2 hour (1 hour = 3,600 s) Al3+(aq) + 3e- ⟶ Al(s) A. 0.000839 g B. 2.20 g C. 0.302 g D. 0.625 g E. 0.906 g
Given: 2H+(aq)+2e– ⇌H2(g);E°=0.00 Li+(aq)+e– ⇌Li(s);E°=–3.04V F2(g)+2e– ⇌2F–(aq);E°=2.87 Al3+(aq)+3e– ⇌Al(s);E°=–1.66V Pb2+(aq)+2e– ⇌Pb(s);E°=–0.13V Under standard-state conditions, which is the strongest oxidizing agent? Select one: a. Pb2+ b. Al3+ c. F2 d. Li+ e.H+
Aluminum oxidizes according to the following equation: 4 Al + 3 O2 -> 2 AL2 O3. If 0.048 mol of Al is placed into a container with 0.030 mol O2, what are the limiting and excess reactants? Based on the previous question, how many moles of excess reactant remain?
Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(s) + 3H2(g) If 12.9 g of aluminum reacts with excess sulfuric acid, and 62.4 g of Al2(SO4)3 are collected, what is the percent yield of Al2(SO4)3?