Answer:
30
Explanation:
Given that;
the compound contains nitrogen and oxygen in the ratio 1:1;
We can say the compound is NO
Now,
Molecular mass of NO;
Molar mass of N = 14g/mol
Molar mass of O = 16g/mol
Molecular mass of NO = 14 + 16 = 30g/mol
Answer:
The answer to the question is
The equilibrium partial pressure (atm) of ammonia, assuming that some solid NH₄HS remains 0.26 atm.
Explanation:
To solve the question, we write out the chemical equation as follows
NH₄HS (s) ⇄ NH₃ (g) + H₂S (g)
From the above equation, it is observed that only the gaseous products contribute to the partial pressure
Kp =PNH₃·PH₂S where at Kp = 0.070 and PNH₃, PH₂S are the partial pressures of the gases
However since the number of moles of both gases are equal, therefore by Avogadro's law PNH₃ = PH₂S
Then PNH₃ = √(0.07) = PH₂S = 0.2645 atm. ≅ 0.26 atm.
