In order to maintain neutrality, the negatively charged ions in the salt bridge will migrate into the anodic half-cell. A similar (but reversed) situation is found in the cathodic cell.
<h3>
What purpose does a salt bridge serve in an oxidation process?</h3>
Anions (negatively charged particles) are added to the solution of the oxidation half of the cell by the salt bridge, and cations (positively charged particles) are added to the solution of the reduction half of the reaction.
<h3>
What purpose does the salt bridge serve in a galvanic cell?</h3>
For instance, KCl, AgNO3, etc. In a galvanic cell, such as a voltaic cell or Daniel cell, salt bridges are typically used. A salt bridge's primary job is to assist in preserving the electrical neutrality of the internal circuit. Additionally, it aids in keeping the cell's response from reaching equilibrium.
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Answer:
Answered
Explanation:
1)False, electron carriers are not located at ribosomes.
2) True, ATP is the common intermediate between catabolic and anabolic pathways.
3)False, ATP is used for the long-term storage of energy and so is often not found in storage granules.
4) True, Anaerobic organisms are capable of generating ATP via respiration.
5) True , ATP can be generated by the flow of protons across protein channels.
Atomic radii increase when going down a group and decreases when going towards the anion periods. So A and D.
<h3>
Answer:</h3>
0.387 J/g°C
<h3>
Explanation:</h3>
- To calculate the amount of heat absorbed or released by a substance we need to know its mass, change in temperature and its specific heat capacity.
- Then to get quantity of heat absorbed or lost we multiply mass by specific heat capacity and change in temperature.
- That is, Q = mcΔT
in our question we are given;
Mass of copper, m as 95.4 g
Initial temperature = 25 °C
Final temperature = 48 °C
Thus, change in temperature, ΔT = 23°C
Quantity of heat absorbed, Q as 849 J
We are required to calculate the specific heat capacity of copper
Rearranging the formula we get
c = Q ÷ mΔT
Therefore,
Specific heat capacity, c = 849 J ÷ (95.4 g × 23°C)
= 0.3869 J/g°C
= 0.387 J/g°C
Therefore, the specific heat capacity of copper is 0.387 J/g°C
