Why does aluminium oxide (Al2O3) have a higher melting point than sodium oxide (Na2O)?
1 answer:
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Answer: (C) conservation of matter
Solution: Law of conservation of matter or mass states that' total mass of the reactants should always be equal to the total mass of the product that is the total mass is remained conserved in a chemical reaction.
A balanced chemical equation always follow this law.
For example:
Mass of hydrogen = 1 g/mol
Mass of Oxygen = 16 g/mol
Total mass on the reactants = 2(2×1)+(2×16)= 36g/mol
Total mass on the product side = 2[(2×1) +16] = 36 g/mol
As,
Mass on reactant side = Mass on the product side
Therefore, a balanced chemical reaction follows Law of Conservation of mass.
If the coulombs are supplied at 1.44 V, then 4.766 × 10¹¹ joules are produced.
(a) The reaction is
2H₂O + 2e⁻ → H₂ + 2OH⁻
According to the reaction, 2 moles of electrons flow per mole of reaction,
(b) Given
T = 25°C
Change Celsius into Kelvin
T = 25°C
= (25 + 273 ) K
= 298 K
<h3>What is Ideal Gas Law ?</h3>It is expressed as
PV = nRT
Hence ,
n =
=
= 1.7176 ×10⁶ mole
Now, From the given reaction we can say that ,1 mole of H₂ is produced by 2 moles of electron
Hence, 1.7176 × 10⁶ mole of H₂ is produced by
= 2 × 1.7176 × 10⁶ moles of electron
= 3.435 ×10⁶ moles of electron
We know that
charge = moles of electron × F
= (3.435 ×10⁶ × 96500) C
= 3.31 × 10¹¹ C
(c) We know that,
Voltage = =
1.44 V =
Energy = 1.44 V × 3.31 × 10¹¹ C
= 4.766 × 10¹¹ Joules
Thus from the above conclusion we can say that, coulombs are supplied at 1.44 V, then 4.766 × 10¹¹ joules are produced.
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Question : Car manufacturers are developing engines that use H₂ as fuel. In Iceland, Sweden, and other parts of Scandinavia countries, where hydroelectric plants produce inexpensive electric power, the H₂ can be made industrially by the electrolysis of water.
a) How many moles of electrons flow per mole of reaction ?
b) How many coulombs are needed to produce 3.53X10⁶ L of H₂ gas at 12.0 atm and 25°C.
c) If the coulombs are supplied at 1.44 V, how many joules are produced?