电极制备及电池电动势的测定

1、实实验验四四 电电极极的的制制备备及及其其电电动动势势的的测测定定（白色区域为输入数据区域，其它地方均为自动生成数据）班级：学号：姓名：同组实验者：实验时间：报告成绩：原电池:Zn(s) | ZnSO4 (a1) | CuSO4 (a2) | Cu(s)原电池:电池反应：Zn ( s) +CuSO4 (b2) ZnSO4 (b1)+ 2Cu(s)电池反应：b1=0.01 mol.dm- 3r- =0.387z= 2b1=b2=0.01 mol.dm- 3r+ =0.4b2=T= 291.15 KT=正极E+ = E+-(RT/zF)ln(1/aCu2+) =0.2707正极负极E- = E-(

2、RT/zF)ln(1/aZn2+) =-0.8327负极理论计算值：E= E+ - E- =1.1034理论计算值：实验测定值：E= 1.079864实验测定值：相对误差Er=2.13%相对误差原电池:Zn(s) | ZnSO4 (a1) | KCl (饱和) |Hg2Cl2, Hg原电池:电池反应：Zn ( s) +Hg2Cl2 (s) Zn2- (b1)+ 2Hg(s) + 2Cl-电池反应：b1=0.01 mol.dm- 3r- =0.387z= 2b1=T= 291.15 KT=正极E+ = (查表4-3不同温度甘汞电极电位)0.2483正极负极E- = E-(RT/zF)ln(1/a

3、Zn2+) =-0.8327负极理论计算值：E= E+ - E- =1.0810理论计算值：实验测定值：E= 1.064675实验测定值：相对误差Er=1.51%相对误差原电池:Hg2Cl2, Hg |KCl (饱和) | CuSO4 (a2) | Cu(s)原电池:电池反应：Hg ( s) +Cu2+ + 2Cl- (饱和) Hg2Cl2 (s) + 2Cu(s)电池反应：b2=0.01 mol.dm- 3r+ =0.4z= 2b2=T= 291.15 KT=正极E+ = E+-(RT/zF)ln(1/aCu2+) =0.2707正极负极E- = (查表4-3不同温度甘汞电极电位)0.248

4、3负极理论计算值：E= E+ - E- =0.0224理论计算值：实验测定值：E= 0.017397实验测定值：相对误差Er=22.47%相对误差思考题：1. 为什么不能用伏特计测量电池的电动势？答：2. 测电动势为何要用盐桥？答：教师评语：Zn(s) | ZnSO4 (a1) | CuSO4 (a2) | Cu(s)Zn ( s) +CuSO4 (b2) ZnSO4 (b1)+ 2Cu(s)0.1 mol.dm- 3r- =0.15z= 20.1 mol.dm- 3r+ =0.16291.15 KE+ = E+-(RT/zF)ln(1/aCu2+) =0.2881E- = E-(RT/zF)

5、ln(1/aZn2+) =-0.8157E= E+ - E- =1.1038E=1.82445Er=65.29%Zn(s) | ZnSO4 (a1) | KCl (饱和) |Hg2Cl2, HgZn ( s) +Hg2Cl2 (s) Zn2- (b1)+ 2Hg(s) + 2Cl-0.1 mol.dm- 3r- =0.15z= 2291.15 KE+ = (查表4-3不同温度甘汞电极电位) 0.2438E- = E-(RT/zF)ln(1/aZn2+) =-0.8157E= E+ - E- =1.0595E=1.51867Er=43.34%Hg2Cl2, Hg |KCl (饱和) | CuSO4 (a2) | Cu(s)Hg ( s) +Cu2+ + 2Cl- (饱和) Hg2Cl2 (s) + 2Cu(s)0.1 mol.dm- 3r+ =0.16z= 2291.15 KE+ = E+-(RT/zF)