Answer:
This occurs when one atom has a higher electronegativity than the atom it is sharing with.
At constant temperature and pressure, If the amount of gas increases to the given value, its volume also increases to 39 mL.
<h3>What is Avogadro's law?</h3>
Avogadro's law states that "equal volumes of all gases, at the same temperature and pressure, have the same number of molecules."
It is expressed as;
V₁/n₁ = V₂/n₂
Given the data in the question;
- Initial amount of gas n₁ = 5.4moles
- Initial volume v₁ = 34mL = 0.034L
- Final amount of gas n₁ = 6.2moles
We substitute our values into the expression above.
V₁/n₁ = V₂/n₂
V₁n₂ = V₂n₁
V₂ = V₁n₂ / n₁
V₂ = (0.034L × 6.2moles) / 5.4moles
V₂ = 0.2108molL / 5.4mol
V₂ = 0.039L
V₂ = 39 mL
Therefore, at constant temperature and pressure, If the amount of gas increases to the given value, its volume also increases to 39 mL.
Learn more about Avogadro's law here: brainly.com/question/15613065
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Answer:
6.2g of NaBr are produced
Explanation:
The reaction of HBr with NaOH occurs as follows:
HBr + NaOH → NaBr + H2O
<em>Where 1 mole of each reactant produce 1 mole of NaBr</em>
To solve this question we need to find the moles of each reactant using their molar mass. With moles we can find limiting reactant and the moles (And mass) of NaBr produced, as follows:
<em>Moles HBr -Molar mass: 80.9119g/mol)-</em>
4.9g * (1mol/80.9119g) = 0.0606 moles HBr
<em>Moles NaOH -Molar mass: 40g/mol-</em>
3.86g * (1mol/40g) = 0.0965 moles NaOH
As the reaction is 1:1 and the moles of HBr < Moles NaOH, the limiting reactant is HBr and moles of NaBr produced are 0.0606 moles.
The mass of NaBr (Molar mass: 102.894g/mol) is:
0.0606 moles * (102.894g/mol) =
<h3>6.2g of NaBr are produced</h3>