Answer:
52.2 g
Explanation:
Step 1: Write the balanced equation
3 KOH + H₃PO₄ ⟶ K₃PO₄ + 3 H₂O
Step 2: Calculate the moles corresponding to 89.7 g of KOH
The molar mass of KOH is 56.11 g/mol.
89.7 g × 1 mol/56.11 g = 1.60 mol
Step 3: Calculate the moles of H₃PO₄ needed to react with 1.60 moles of KOH
The molar ratio of KOH to H₃PO₄ is 3:1. The moles of H₃PO₄ needed are 1/3 × 1.60 mol = 0.533 mol.
Step 4: Calculate the mass corresponding to 0.533 moles of H₃PO₄
The molar mass of H₃PO₄ is 97.99 g/mol.
0.533 mol × 97.99 g/mol = 52.2 g
Answer:
The rate at which 
is being produced is 0.0228 M/s.
The rate at which 
is being consumed is 0.0912 M/s.
Explanation:
Rate of the reaction : R
![R=\frac{-1}{4}\frac{d[PH_3]}{dt}=\frac{1}{6}\frac{d[H_2]}{dt}=\frac{1}{1}\frac{d[P_4]}{dt}](https://tex.z-dn.net/?f=R%3D%5Cfrac%7B-1%7D%7B4%7D%5Cfrac%7Bd%5BPH_3%5D%7D%7Bdt%7D%3D%5Cfrac%7B1%7D%7B6%7D%5Cfrac%7Bd%5BH_2%5D%7D%7Bdt%7D%3D%5Cfrac%7B1%7D%7B1%7D%5Cfrac%7Bd%5BP_4%5D%7D%7Bdt%7D)
The rate at which hydrogen is being formed = ![\frac{d[H_2]}{dt}=0.137 M/s](https://tex.z-dn.net/?f=%5Cfrac%7Bd%5BH_2%5D%7D%7Bdt%7D%3D0.137%20M%2Fs)
![R=\frac{1}{6}\frac{d[H_2]}{dt}](https://tex.z-dn.net/?f=R%3D%5Cfrac%7B1%7D%7B6%7D%5Cfrac%7Bd%5BH_2%5D%7D%7Bdt%7D)
The rate at which is being produced:
![R=\frac{1}{1}\frac{d[P_4]}{dt}](https://tex.z-dn.net/?f=R%3D%5Cfrac%7B1%7D%7B1%7D%5Cfrac%7Bd%5BP_4%5D%7D%7Bdt%7D)
![0.0228 M/s=\frac{1}{1}\frac{d[P_4]}{dt}](https://tex.z-dn.net/?f=0.0228%20M%2Fs%3D%5Cfrac%7B1%7D%7B1%7D%5Cfrac%7Bd%5BP_4%5D%7D%7Bdt%7D)
The rate at which is being consumed :
![R=\frac{-1}{4}\frac{d[PH_3]}{dt}](https://tex.z-dn.net/?f=R%3D%5Cfrac%7B-1%7D%7B4%7D%5Cfrac%7Bd%5BPH_3%5D%7D%7Bdt%7D)
![0.0228 M/s\times 4=\frac{-1}{1}\frac{d[PH_3]}{dt}](https://tex.z-dn.net/?f=0.0228%20M%2Fs%5Ctimes%204%3D%5Cfrac%7B-1%7D%7B1%7D%5Cfrac%7Bd%5BPH_3%5D%7D%7Bdt%7D)
![\frac{-1}{1}\frac{d[PH_3]}{dt}=0.912 M/s](https://tex.z-dn.net/?f=%5Cfrac%7B-1%7D%7B1%7D%5Cfrac%7Bd%5BPH_3%5D%7D%7Bdt%7D%3D0.912%20M%2Fs)
Answer:
380 mL is the new volume
Explanation:
At constant pressure.
V₁ / T₁ = V₂ / T₂
Temperature must be in Absolute Values (T°K = T°C + 273)
-125°C + 273 = 148 K
31°C + 273 = 304 K
185 mL / 148 K = V₂ / 304 K
V₂ = (185 mL / 148 K) . 304 K → 380 mL
