The formation of CsCl from Cs(s) and Cl2(g) involves the following steps: Cs(s)→Cs(g) 12Cl2(g)→Cl(g) Cs(g)→Cs+(g)+e− Cl(g)+e−→Cl−(g) Cs+(g)+Cl−(g)→CsCl(s) Which of these steps absorb energy and which release energy?
Cs(s)→Cs(g)
Changing from solid to gas will absorb energy
12Cl2(g)→Cl(g)
breaking bond will absorb energy
Cs(g)→Cs+(g)+e−
This is ionisation reaction. This will absorb energy
Cl(g)+e−→Cl−(g)
This will release energy.
Cs+(g)+Cl−(g)→CsCl(s)
Formation of bond releases energy
The formation of CsCl from Cs(s) and Cl2(g) involves the following steps: Cs(s)→Cs(g) 12Cl2(g)→Cl(g) Cs(g)→Cs+(g)+e− Cl(g)+e−→Cl−(g)...
The formation of CsCl from Cs(s) and Cl2(g) involves the following steps: Cs(s)?Cs(g) 12Cl2(g)?Cl(g) Cs(g)?Cs+(g)+e? Cl(g)+e??Cl?(g) Cs+(g)+Cl?(g)?CsCl(s) Which of these steps absorb energy and which release energy?
Which compound has the bigger lattice energy? Lici Lil Rb20 KO CsCl Cs,S
Based on the following information, Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.36 V Mg2+(aq) + 2 e- → 2 Mg(s) E° = -2.37 V which of the following chemical species is the strongest reducing agent? A. Cl2(g) B. Mg2+(aq) C. Mg(s) D. Cl-(aq)
Which equation represents the heat of formation, ∆Hf, for MgCl2? Mg2+(aq) + 2 Cl– → MgCl2(s) Mg(s) + 2 Cl(g) → MgCl2(s) MgCl2(s) → Mg2+(aq) + 2 Cl–(aq) Mg(s) + Cl2(g) → MgCl2(s)
Consider the following gas phase reaction: 12(g) + Cl2(g) →21C1(e) If 4.46 liters of Cl(s) gas at 119°C and 0.996 atm is used, what volume of ICl(g) gas will be formed if it is collected at 168°C and 1.21 atm? liters Submit Answer Retry Entire Group 1 more group attempt remaining
4. a) Determine Eº for the cell Pt (s) | Cl2 (g) | Cl− (aq) || Pb2+ (aq), H+ (aq) | PbO2 (s). b) What is the Standard Gibbs free energy of this reaction?
Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s) The reaction utilized by this cell is Question 8 options: Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) 2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq)
The proposed mechanism for a reaction is Cl2 => Cl+ + Cl- Slow Cl- + H2S => HCl + HS- Fast Cl+ + HS- => HCl + S Fast Which of the following would be a rate law for the reaction? A. rate = k[Cl2] B. rate = k[Cl2][H2S] C. rate = k[Cl2]1/2[H2S] D. rate = k[Cl-][H2S] E. rate = [Cl+][Cl-]
Which part(s) of the reaction Cl2(g) <---> 2 Cl(g) will be favored by an increase in the total pressure (resulting in compression)? Please explain. a.) neither is favored b.) unable to determine c.) products d.) reactants
Balance the following redox reaction in basic solution. Cl (aq)+Cro (aq) - Cl2(g)+Cr(OH)3(s) Cl (aq) Cro (aq) C,(g) Cr(OH), (s)