The balanced equation for the reaction is ;
2Zn + O2 —> 2ZnO
The stoichiometry of O2 to ZnO is 1:2
The mass of ZnO formed - 358.5 g
The number of moles formed - 358.5 g / 81.4 g/mol = 4.4 moles
Therefore number of O2 moles reacted = 4.4 moles /2 = 2.2 mol
Mass of O2 reacted = 2.2 mol x 32 g/mol = 70.4 g
I don't know but I think that 0.02 g/mL is 20 g/L because you multiply the 0.02 by a 100. That's how you get the Gram liter
Atomic # 64
electronic configuration is *[Xe] 6s^2 4f^8
n = 4
ℓ = 3
mℓ<span> = -3</span>
ms<span> = -½</span>
Answer:
The pressure is 58.75 atm.
Explanation:
From Vanderwaal's equation,
P = nRT/(V-nb) - n^2a/V^2
n is the number of moles of SO2 = mass/MW = 500/64 = 7.81 mol
R is gas constant = 0.0821 L.atm/mol.K
T is temperature of the vessel = 633 K
V is volume of the vessel = 6.3 L
a & b are Vanderwaal's constant = 6.865 L^2.atm/mol^2 and 0.0567 L/mol respectively.
P = (7.81×0.0821×633)/(6.3 - 7.81×0.05679) - (7.81^2 × 6.865)/6.3^2 = 69.30 - 10.55 = 58.75 atm
Answer:
526.85K
Explanation:
Based on Charles's law, the volume of a gas is directly proportional to absolute temperature. The formrula is:
V₁ / T₁ = V₂ / T₂
<em>Where 1 represents the initial state and 2 the final state of the gas</em>
Using the values of the problem:
V₁ = 10.0L
T₁ = 127°C + 273.15K = 400.15K
V₂ = 20.0L
Thus, replacing in the formula:
10.0L / 400.15K = 20.0L / T₂
T₂ = 800K
In Celsius:
800K - 273.15 =<em> 526.85K</em>
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