The chemical formula depends on the type of acids it is. Acidic rain is a complex mixture of nitrous, nitric, sulfurous and sulfuric acids which all combine to lower the pH.
Answer:
The initial temperature is 499 K
Explanation:
Step 1: Data given
initial volume = 12 cm3 = 12 mL
Final volume = 7 cm3 = 7mL
The final temperature = 18 °C = 291 K
Step 2: Calculate the initial temperature
V1/T1 = V2/T2
⇒with V1 = the initial volume = 0.012 L
⇒with T1 = the initial volume = ?
⇒with V2 = the final volume 0.007 L
⇒with T2 = The final temperature = 291 K
0.012 / T1 = 0.007 / 291
0.012/T1 = 2.4055*10^-5
T1 = 0.012/2.4055*10^-5
T1 = 499 K
The initial temperature is 499 K
Answer: The equilibrium concentration of 
will be much smaller than the equilibrium concentration of 
, because Keq<<1
Explanation:
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as 
K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.
For the given chemical reaction:
The expression for is written as:
![K=\frac{[H_3O^+]\times [BrO^-]}{[HBrO]}](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BH_3O%5E%2B%5D%5Ctimes%20%5BBrO%5E-%5D%7D%7B%5BHBrO%5D%7D)
Concentration of pure solids and liquids is taken as 1.
Thus as 
, That means the concentration of products is less as the reaction does not proceed much towards the forward direction.
Answer:
C. 2O₃ ⇌ 3O₂
Explanation:
Kp is the equilibrium constant calculated from the partial pressures of a gas-phase reaction equation.
For a general gas-phase reaction aA + bB ⇌ nC + xD
the expression for the Kp = (pC)ⁿ(pD)ˣ / (pA)ᵃ(pB)ᵇ
where pA = partial pressure of A; pB = partial pressure of B; pC = partial pressure of C; pD = partial pressure of D
From the given reaction in equilibrium; N₂ + 3H₂ ⇌ 2NH₃
Kp = (pNH₃)² / (pN₂)¹ * (pH₂)³ = 4/7
(pNH₃)² / (pN₂)¹ * (pH₂)³ = (2)²/ (1)¹ * (3)³
Therefore, number of mole of reactants and products is equivalent to partial pressure.
A. 2SO₂ ⇌ O₂ + 2SO₃
pSO₂ = 2, pO₂ = 1, pSO₃ = 2,
Kp = 2²/ (2² * 1²) = 4/4 = 1
B. N₂O₄ ⇌ 2NO₂
pN₂O₄ = 1, pNO₂ = 2
Kp = 2²/1² = 4
C. 2O₃ ⇌ 3O₂
pO₃ = 2, pO₂ = 3
Kp = 3³/2² = 27/4
D. PCl₅ ⇌ PCl₃ + Cl₂
pPCl₅ = 1, pPCl₃ = 1, pCl₂ = 1
Kp = (1¹ * 1¹) / 1¹ = 1
