Why are non-standard conditions crucial in chemical reactions?

Understanding Galvanic Cells and Non-Standard Conditions

Interactive Video
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Chemistry, Science
•
11th Grade - University
•
Hard

Sophia Harris
FREE Resource
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10 questions
Show all answers
1.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
They are rarely encountered in real-life reactions.
They simplify the calculation of cell potential.
They provide a theoretical framework for standard conditions.
Chemical reactions are always at non-standard conditions.
2.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
Who developed the Nernst equation and in which year?
Albert Einstein in 1905
Marie Curie in 1898
Dmitri Mendeleev in 1869
Walther Nernst in 1887
3.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What happens to the cell potential when Q is greater than 1?
It decreases below the standard cell potential.
It becomes zero immediately.
It remains the same as the standard cell potential.
It increases above the standard cell potential.
4.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What is the relationship between cell potential and equilibrium constant at equilibrium?
Cell potential is negative.
Cell potential is equal to the equilibrium constant.
Cell potential is zero.
Cell potential is maximum.
5.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What happens to the cell potential when Q is less than 1?
It decreases below the standard cell potential.
It remains the same as the standard cell potential.
It increases above the standard cell potential.
It becomes zero immediately.
6.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How does adding sodium hydroxide to the cathode compartment affect the cell potential?
It decreases the cell potential.
It doubles the cell potential.
It has no effect on the cell potential.
It increases the cell potential.
7.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How does increasing the molarity of zinc ions affect the cell potential?
It doubles the cell potential.
It has no effect on the cell potential.
It decreases the cell potential.
It increases the cell potential.
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