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miv72 [106K]
3 years ago
9

What is the temperature of 1.2 moles of helium gas at 2.57 ATM if it occupies 15.5L of volume

Chemistry
1 answer:
agasfer [191]3 years ago
8 0
We will assume helium to behave as an ideal gas and apply the ideal gas law:
PV = nRT
For pressure measured in atmospheres and volume measured in liters, the value of the molar gas constant is 0.082. Therefore:
T = PV / nR
T = (2.57 x 15.5) / (1.2 x 0.082)
T = 404.8 Kelvin
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If 125g of KClO3 is heated, what is the total mass of the products?​
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Given parameters:

Mass of KClO₃  = 125g

Unknown:

Total mass of the products = ?

When  KClO₃ is heated, it thermally decomposes to KCl and O₂ according to the chemical equation below;

               2KClO₃  →  2KCl + 3O₂

All chemical equations obeys the law of conservation of matter and with this regard, we know that the amount of reactants used is the same as that of the product.

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Now to find the masses of each product,

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Total mass of products = mass of KCl + Mass of O₂ = 75.99g + 48.96g

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This value is approximately the same as that of mass of  KClO₃

 

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