The last statement is correct...
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The number of moles of silver oxide (I) needed to produce 4 moles of silver is 2 moles
<h3>Stoichiometry </h3>
From the question, we are to determine the number of moles of silver oxide (I) needed to produce 4 moles of silver
First, we will write the balaced chemical equation for the decomposition of silver oxide (I)
2Ag₂O(s) → 4Ag(s) + O₂(g)
This means, 2 moles of silver oxide (I) [Ag₂O] decomposes to give 4 moles of <u>silver </u>and 1 mole of oxygen gas.
From the <em>balanced chemical equation</em>, it is easy to deduce the number of moles of silver oxide (I) that would give 4 moles of silver.
Hence, the number of moles of silver oxide (I) needed to produce 4 moles of silver is 2 moles
Learn more on Stoichiometry here: brainly.com/question/18834543
When H is positive and S is negative
Answer:
2.1 moles of water formed.
Explanation:
Given data:
Moles of water formed = ?
Moles of Ni(OH) = 4.20 mol
Solution:
Chemical equation:
2Ni(OH) → Ni₂O + H₂O
Now we will compare the moles of Ni(OH) with water.
Ni(OH) : H₂O
2 : 1
4.20 : 1/2×4.20 = 2.1 mol
2.1 moles of water formed.
Answer: D. An increase in entropy
Explanation:
Entropy is the measure of randomness or disorder of a system. If a system moves from an disordered arrangement to an ordered arrangement, the entropy is said to increase and vice versa.
For a reaction to be spontaneous, the enthalpy of the solution must decrease and the entropy must increase.
To overcome a positive enthalpy of solution and allow a solid solute to dissolve in water, an increase in entropy would make the reaction spontaneous as the system would move to a more disordered state.
