Answer:
2Ag⁺ (aq) + 2OH⁻ (aq) → Ag₂O (s) + H₂O (l)
Explanation:
Step 1: RxN
2AgNO₃ + 2NaOH → Ag₂O + 2NaNO₃ + H₂O
Step 2: Define states of matter
2AgNO₃ (aq) + 2NaOH (aq) → Ag₂O (s) + 2NaNO₃ (aq) + H₂O (l)
Step 3: Total Ionic Equation
2Ag⁺ (aq) + 2NO₃⁻ (aq) + 2Na⁺ (aq) + 2OH⁻ (aq) → Ag₂O (s) + 2Na⁺ (aq) + 2NO₃⁻ (aq) + H₂O (l)
Step 4: Cancel out spectator ions
2Ag⁺ (aq) + 2OH⁻ (aq) → Ag₂O (s) + H₂O (l)
From ideal gas equation that is PV=nRT
n(number of moles)=PV/RT
P=760 torr
V=4.50L
R(gas constant =62.363667torr/l/mol
T=273 +273=298k
n is therefore (760torr x4.50L) /62.36367 torr/L/mol x298k =0.184moles
the molar mass of NO2 is 46 therefore density= 0.184 x 46=8.464g/l
The arrows represent the movement of starting substances
The proton has a positive charge.
