Answer:
Mass = 75.6 g
Explanation:
Given data:
Temperature of gas = 17°C
Volume of gas = 575 mL
Pressure of gas = 85000 mmHg
Mass of gas = ?
Solution:
Temperature of gas = 17°C (17+273 =290 K)
Volume of gas = 575 mL (575/1000 = 0.575 L)
Pressure of gas = 85000 mmHg (85000/760 = 111.8 atm)
Formula:
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
111.8 atm × 0.575 L = n×0.0821 atm.L/ mol.K × 290 K
64.285 atm. L = n×23.809 atm.L/ mol
n = 64.285 atm. L / 23.809 atm.L/ mol
n = 2.7 mol
Mass of nitrogen gas:
Mass = number of moles × molar mass
Mass = 2.7 mol × 28 g/mol
Mass = 75.6 g
Answer:
Synthesis Reaction
General Formulas and Concepts:
<u>Chemistry - Reactions</u>
- Synthesis Reactions: A + B → AB
- Decomposition Reactions: AB → A + B
- Single-Replacement Reactions: A + BC → AB + C
- Double-Replacement Reactions: AB + CD → AD + BC
Explanation:
<u>Step 1: Define</u>
RxN: 2Na + I₂ → 2NaI
<u>Step 2: Identify</u>
2Na + I₂ → 2NaI
A + B → AB
Synthesis Reaction