Answer: Total pressure = 7293.2 torr or 9.60 atm
Explanation:
<em>Total pressure = partial pressure of nitrogen + partial pressure of oxygen</em>
The partial pressure due to nitrogen is determined using the equation of Gay-Lussac's law: <em>P₁/T₁=P₂/T₂</em>
P₁ = 760 torr = 1atm, T₁ = 28∘C = (273+28)K = 301k, P₂ = ?, T₂ = 310∘C =(310+273)K = 583K
P₂ = P₁ T₂/ T₁
P₂ = 760 * 583 / 301 = 1472.03 torr
The pressure due to Oxygen gas produced is calculated thus:
Balanced equation of the decomposition of Ag₂O at s.t.p. is as follows;
2Ag₂O ----> 4Ag + O₂(g)
2 moles of Ag₂O produces 1 mole of O₂
molar mass of Ag₂O = (2*108 + 16)g = 232g/mol
molar volume of gas at s.t.p. = 22.4L
2*232g i.e. 464g of Ag₂O produces 22.4L of O₂
5.57g of Ag₂O will produce 5.57g*22.4L/464g = 0.269L or 269mL of O₂
Using the General gas equation P₁V₁/T₁=P₂V₂/T₂
P₁ = 1atm = 760 torr, V₁ = 269mL, T₁=273K, P₂ = ?, V₂= 75mL, T₂ = 583K
P₂ = P₁V₁T₂/V₂T₁
P₂ = 760*269*583 / 75*273
P₂ = 5821.17 torr
Total pressure = (1472.03 + 5821.17) torr
Total pressure = 7293.2 torr or 9.60 atm
