Option (a) is correct.
A reducing agent is the one which loses electrons to other substance.
Here, Zn has oxidation number 0 in the L.H.S of the equation, but on R.H.S its oxidation number is +2 i.e. it Zn has donated two of its electrons to
.
Hence, Zn is the reducing agent here.
I will list them from alkaline with the lowest boiling point and alkaline with the highest.
1. C2H6
2. C9H20
3. C11H24
4. C16H34
5. C20H42
6. C32H66
7. C150H302
I have taken a quiz similar to this before and can assure you this is correct and is primarily because of the number of Carbons and Hydrogens within this. More Carbons and Hydrogens causes Boiling Points to increase because of stronger bonds.
When a substance absorbs thermal energy, it partitions some as potential and some as kinetic energy. Specific heat is an expression related to the quantity of heat a substance stores as potential energy; the remainder is absorbed as kinetic which causes the temperature to increase - recall that temperature is a measure of average kinetic energy.
When specific heat is low, most of the energy is partitioned as kinetic energy and the substance will experience the greatest temperature change.
So rather than calculating the change in temperature, we can simply inspect the specific heats. The one with the lowest will experience the greatest temperature change. We could also compare the specific heats: Al = .897/.385 ==> 2.3, Fe = .452/.385 = 1.2, Cu = .385/.385 = 1. We can expect Copper's temperature change to be 2.3 times larger than Aluminum's and 1.2 times larger than Iron's.
Answer:
Explanation:
Given: Entropy of surrounding: ΔSsurr = ?
Temperature: T= 355 K
The change in enthalpy of reaction: ΔH = -114 kJ
Pressure: P = constant
As we know, ΔH = -114 kJ ⇒ negative
Therefore, the given reaction is an exothermic reaction
Therefore, Entropy of surrounding at <em>constant pressure</em> is given by,
<u><em>In the given reaction:</em></u>
2NO(g) + O₂(g) → 2NO₂(g)
As, the number of moles of gaseous products is less than the number of moles of gaseous reactants.
As we know, <em>for a spontaneous process, that the total entropy should be positive.</em>
<u>Therefore, at the given temperature,</u>
- if
then the given reaction is spontaneous
- if
then the given reaction is non-spontaneous
The answer for your question is B
