I cant see the chemical reaction taking place, and what is the evidence to support it
Answer:
Explanation:
<em>Given: </em>
P1 = 78.89 ATM
V1 = 12 litres
T1 = 70° C= 343.15 K
V2 = 10 litres
T2 = 95°C= 368.15 K
<em>To find:</em>
P2 = ?
<em>Solution:</em>
Using ideal gas equation,
Since the number of moles & Universal gas constant (R) is constant, the final relation that would be derived between initial & final variables.
<em>(The only unit conversion needed is temperature because it was an addition factor, for other variables it will be cancelled out) </em>
Answer:
N₃O₆
Step-by-step explanation:
Data:
EF = NO₂
MM = 138.02 g/mol
Calculations:
EF Mass = (14.01 + 32.00) u
EF Mass = 46.01 u
The molecular formula is an integral multiple of the empirical formula.
MF = (EF)ₙ
n = MF Mass/EF Mass
n = 138.02 u/46.01 u
n = 3.000 ≈3
MF = (NO₂)₃
MF = N₃O₆