The molar mass of a gas that moves 1.25 times as fast as CO2 is 28.16 g.
<h3>
Molar mass of the gas</h3>
The molar mass of the gas is determined by applying Graham's law of diffusion.
R₁√M₁ = R₂√M₂
R₁/R₂ = √M₂/√M₁
R₁/R₂ = √(M₂/M₁)
where;
- R₁ is rate of the CO2 gas
- M₁ is molar mass of CO2 gas
- R₂ is rate of the second gas
- M₂ is the molar mass of the second gas
R₁/1.25R₁ = √(M₂/44)
1/1.25 = √(M₂/44)
0.8 = √(M₂/44)
0.8² = M₂/44
M₂ = 0.8² x 44
M₂ = 28.16 g
Thus, the molar mass of a gas that moves 1.25 times as fast as CO2 is 28.16 g.
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Answer:
Explanation:
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In this case, since the equilibrium expression for the considered equation is:
Which can be written in terms of the reaction extent and the ICE chart and the initial concentrations of 0.453 M as shown below:
We can solve for x as follows:
In such a way, we obtain the following concentrations at equilibrium:
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Answer:
(<em>i) Concentrated HNO3 can be stored and transported in aluminium containers as it reacts with aluminium to form a thin protective oxide layer on the aluminium surface. This oxide layer renders aluminium passive. (ii) Sodium hydroxide and aluminium react to form sodium tetrahydroxoaluminate(III) and hydrogen gas.</em>