What will be the total pressure in the chamber after the reaction?

[匿名]

2021-02-09 2:44 pm

Consider the reaction between silicon monoxide and hydrogen to form the gas H2SiO. How much H2SiO can be generated by the reaction of 23.2 g of silicon monoxide and 5.20 g of hydrogen gas by the reaction below in a 7.00 L chamber at 125 oC? What will be the total pressure in the chamber after the reaction?

更新1:

125 oC = 125 Celsius

回答 (1)

Uncle Michael

2021-02-09 4:48 pm

✔ 最佳答案

The melting point of SiO (silicon monoxide) is 1880°C.
At 125°C, SiO exists as a solid.

Molar mass of SiO = (28.09 + 16.00) g/mol = 44.09 g/mol
Molar mass of H₂ (hydrogen gas) = 1.008×2 g/mol = 2.016 g/mol

Initial moles of SiO = (23.2 g) / (44.09 g/mol) = 0.5262 mol
Initial moles of H₂ = (5.20 g) / (2.016 g/mol) = 2.579 mol

Balanced equation of the reaction: H₂(g) + SiO(g) → H₂SiO(g)
Initial moles of H₂ is much greater than initial moles of SiO.
Hence, SiO is the limiting reactant.

After the reaction:
Moles of SiO left = 0 mol
Moles of H₂ gas left = (2.579 - 0.5262) mol
Moles of H₂SiO gas formed = 0.5262 mol
Total moles of gas, n = [(2.579 - 0.5262) + 0.5262] mol = 2.579 mol

PV = nRT, then P = nRT/V
Total pressure in the chamber after the reaction, P
= 2.579 × 0.08206 × (273 + 125) / 7.00 atm
= 12.0 atm

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