can someone pls explain question 13
http://www.boardofstudies.nsw.edu.au/hsc_exams/hsc2003exams/pdf_doc/chemistry_03.pdf
http://www.boardofstudies.nsw.edu.au/hsc_exams/hsc2003exams/pdf_doc/chemistry_03.pdf
2003 hsc question help (1 Viewer)
- Thread starter kr73114
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hscishard
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The last one gives it away. There is no displacement reaction there, so Z is more active than X. The 1st one shows X is more active than Y. So Z>X>Y. D
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MostDefinitelyIncredible
A More active metal displaces a less active metal from solution.
Basically, the more active metal will be more reactive with other metals.
From Diagram 1 - We can tell that Metal X is a more active metal than metal Y because it reacts with Y2+ ions forming deposits of metal Y on metal X. X>Y
From Diagram 2 - Metal Z is more active than metal Y , metal Y deposits on Metal Z as metal Z is more reactive than Metal Y. Z>Y
From Diagram 3 - Metal X is less reactive with Metal Z , this is because a non-active metal cannot displace a more reactive metal. This can be seen as metal Z does not deposit on metal X. Thus Z>X
Overall
X>Y , Z>Y and Z>X
Z>X>Y
Basically, the more active metal will be more reactive with other metals.
From Diagram 1 - We can tell that Metal X is a more active metal than metal Y because it reacts with Y2+ ions forming deposits of metal Y on metal X. X>Y
From Diagram 2 - Metal Z is more active than metal Y , metal Y deposits on Metal Z as metal Z is more reactive than Metal Y. Z>Y
From Diagram 3 - Metal X is less reactive with Metal Z , this is because a non-active metal cannot displace a more reactive metal. This can be seen as metal Z does not deposit on metal X. Thus Z>X
Overall
X>Y , Z>Y and Z>X
Z>X>Y