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Консультация № 190658
06.03.2017, 11:17
0.00 руб.
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1
Здравствуйте! У меня возникли сложности с таким вопросом:
Металлический проводник, изготовленный из олова, погружён в 0,01 М раствор соли SnSO4.
Рассчитать величину относительно электродного потенциала данного электрода. Пользуясь таблицей стандартных электродных потенциалов, составить схему гальванического элемента, в котором рассматриваемый электрод является анодом. Для выбранного гальванического элемента записать уравнения электродных процессов и уравнение электрохимического процесса. Рассчитать величину ЭДС, приняв электродный потенциал катода, равный стандартному. Чему равна стандартная ЭДС?
Металлический проводник, изготовленный из олова, погружён в 0,01 М раствор соли SnSO4.
Рассчитать величину относительно электродного потенциала данного электрода. Пользуясь таблицей стандартных электродных потенциалов, составить схему гальванического элемента, в котором рассматриваемый электрод является анодом. Для выбранного гальванического элемента записать уравнения электродных процессов и уравнение электрохимического процесса. Рассчитать величину ЭДС, приняв электродный потенциал катода, равный стандартному. Чему равна стандартная ЭДС?
Обсуждение
12.03.2017, 12:01
общий
это ответ
Здравствуйте, ospi!
По таблице стандартных электродных потенциалов металлов в водных растворах установим, что потенциал E0(Cu/Cu2+)=+0,340 В>E0(Sn/Sn2+)=-0,136 В. Поэтому в паре металлов олово - медь первый из них более активен, второй - менее активен. Оловянный электрод будет анодом, медный электрод, опущенный в 1М раствор, например, сульфата меди, - катодом.
Схема гальванического элемента такова:
На аноде будет происходить процесс окисления, а на катоде - процесс восстановления, которые описываются следующими уравнениями:
Анодный процесс: Sn-2e=Sn[sup]2+[/sup];
Катодный процесс: Cu[sup]2+[/sup]+2e=Cu.
Уравнение электрохимического процесса: Sn+Cu[sup]2+[/sup]=Sn[sup]2+[/sup]+Cu.
Вычислим потенциал анода по уравнению Нернста:
Вычислим величину ЭДС, приняв электродный потенциал катода, равный стандартному:
Вычислим стандартную ЭДС:
По таблице стандартных электродных потенциалов металлов в водных растворах установим, что потенциал E0(Cu/Cu2+)=+0,340 В>E0(Sn/Sn2+)=-0,136 В. Поэтому в паре металлов олово - медь первый из них более активен, второй - менее активен. Оловянный электрод будет анодом, медный электрод, опущенный в 1М раствор, например, сульфата меди, - катодом.
Схема гальванического элемента такова:
(–)Sn|SnSO[sub]4[/sub]||CuSO[sub]4[/sub]|Cu(+)
На аноде будет происходить процесс окисления, а на катоде - процесс восстановления, которые описываются следующими уравнениями:
Анодный процесс: Sn-2e=Sn[sup]2+[/sup];
Катодный процесс: Cu[sup]2+[/sup]+2e=Cu.
Уравнение электрохимического процесса: Sn+Cu[sup]2+[/sup]=Sn[sup]2+[/sup]+Cu.
Вычислим потенциал анода по уравнению Нернста:
EА=-0,136+(0,059/2)*lg 0,01=-0,136-0,059=-0,195 (В).
Вычислим величину ЭДС, приняв электродный потенциал катода, равный стандартному:
E=E[sub]K[/sub]-E[sub]A[/sub]=+0,340-(-0,195)=0,535 (В).
Вычислим стандартную ЭДС:
E[sup]0[/sup]=E[sup]0[/sup][sub]K[/sub]-E[sup]0[/sup][sub]A[/sub]=+0,340-(-0,136)=0,576 (В).
5
Огромное спасибо)))) За подробный ответ! Очень стыдно за себя, что совсем не знаю химию(((
Об авторе:
Facta loquuntur.
Facta loquuntur.
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