The final temperature, t₂ = 30.9 °C
<h3>Further explanation</h3>
Given
24.0 kJ of heat = 24,000 J
Mass of calorimeter = 1.3 kg = 1300 g
Cs = 3.41 J/g°C
t₁= 25.5 °C
Required
The final temperature, t₂
Solution
Q = m.Cs.Δt
Q out (combustion of compound) = Q in (calorimeter)
24,000 = 1300 x 3.41 x (t₂-25.5)
t₂ = 30.9 °C
Answer: Option (d) is the correct answer.
Explanation:
Steps involved for the given reaction will be as follows.
Step 1:
(fast)
Rate expression for step 1 is as follows.
Rate = k ![[NO]^{2}](https://tex.z-dn.net/?f=%5BNO%5D%5E%7B2%7D)
Step 2: 
This step 2 is a slow step. Hence, it is a rate determining step.
Step 3.
(fast)
Here,
is intermediate in nature.
All the steps are bimolecular and it is a second order reaction. Also, there is no catalyst present in this reaction.
Thus, we can conclude that the statement step 1 is the rate determining step, concerning this mechanism is not directly supported by the information provided.
I believe the answer is A (it was on another Brainly question as well).
Answer:
I think its a double reaction
Explanation:
The volume of H₂ evolved at NTP=0.336 L
<h3>Further explanation</h3>
Reaction
Decomposition of NH₃
2NH₃ ⇒ N₂ + 3H₂
conservation mass : mass reactants=mass product
0.28 NH₃= 0.25 N₂ + 0.03 H₂
2 g H₂ = 22.4 L
so for 0.03 g :
