Answer:
this us a pm interesting question
Explanation:
good job
Answer:

Explanation:
Hello,
In this case, for the given chemical reaction at equilibrium:

The initial concentration of sulfur trioxide is:
![[SO_3]_0=\frac{0.660mol}{4.00L}=0.165M](https://tex.z-dn.net/?f=%5BSO_3%5D_0%3D%5Cfrac%7B0.660mol%7D%7B4.00L%7D%3D0.165M)
Hence, the law of mass action to compute Kc results:
![Kc=\frac{[SO_2]^2[O_2]}{[SO_3]^2}](https://tex.z-dn.net/?f=Kc%3D%5Cfrac%7B%5BSO_2%5D%5E2%5BO_2%5D%7D%7B%5BSO_3%5D%5E2%7D)
In such a way, in terms of the change
due to the reaction extent, by using the ICE method, it is modified as:

In that case, as at equilibrium 0.11 moles of oxygen are present,
equals:
![x=[O_2]=\frac{0.110mol}{4.00L}=0.0275M](https://tex.z-dn.net/?f=x%3D%5BO_2%5D%3D%5Cfrac%7B0.110mol%7D%7B4.00L%7D%3D0.0275M)
Therefore, the equilibrium constant finally turns out:

Best regards.
Answer: I think that the answer was False.
Your answer should be “C.”
MARK ME BRAINLIEST PLEASE!!!!!!
Answer:
1.104 J/g°C
Explanation:
Using Q = m × c × ∆T
Where;
m = mass of substance (g)
c = specific hear capacity (J/g°C)
∆T = change in temperature (°C)
For a colorimeter,
Q(water) = - Q(metal)
m. c. ∆T (water) = - m. c. ∆T (metal)
According to the information provided;
For water:
m = 28.0g
c = 4.184 J/g°C
∆T = (21.23 - 19.73°C)
For the metal:
m = 2.05g
c = ?
∆T = (21.23 - 98.88°C)
m. c. ∆T (water) = - m. c. ∆T (metal)
[28 × 4.184 × (21.23 - 19.73°C)] = -[2.05 × c × (21.23 - 98.88°C)]
[117.152 × 1.5] = -[2.05 × c × (-77.65)]
175.728 = -[-159.1825c]
175.728 = 159.1825c
c = 175.728 ÷ 159.1825
c = 1.104
c = 1.104 J/g°C