Answer:
HI.
Explanation:
- Thomas Graham found that, at a constant temperature and pressure the rates of effusion of various gases are inversely proportional to the square root of their masses.
Rate of effusion ∝ 1/√molar mass.
- <em>(Rate of effusion of O₂) / (Rate of effusion of unknown gas) = (√molar mass of unknown gas) / (√molar mass of O₂).</em>
- An unknown gas effuses at one half the speed of that of oxygen.
∵ Rate of effusion of unknown gas = 1/2 (Rate of effusion of O₂)
∴ (Rate of effusion of O₂) / (Rate of effusion of unknown gas) = 2.
Molar mass of O₂ = 32.0 g/mol.
∵ (Rate of effusion of O₂) / (Rate of effusion of unknown gas) = (√molar mass of unknown gas) / (√molar mass of O₂).
∴ 2.0 = (√molar mass of unknown gas) / √32.0.
(
√molar mass of unknown gas) = 2.0 x √32.0
By squaring the both sides:
∴ molar mass of unknown gas = (2.0 x √32.0)² = 128 g/mol.
∴ The molar mass of sulfur dioxide = 80.91 g/mol and the molar mass of HI = 127.911 g/mol.
<em>So, the unknown gas is HI.</em>
<em></em>
The correct answer is A. AgCl (s) only
The answer is <span>the
reaction will shift to the left (toward the reactants).
Reaction is at equilibrium can be expressed as,
Reactants </span>⇄ products<span>
<span>After coming to the equilibrium, if one condition
is changed, then according to the </span>Le chatelier's Principal,<span> the system
will act to maintain the equilibrium by reducing the effect. As an example, if
we reduce the pressure, then system acts to increase the pressure to maintain
the equilibrium.</span>
<span>Likewise, if we add products into the reaction
which is in equilibrium, the system acts to reduce the effect by promoting the backward
reaction to produce reactants.</span></span>
