Write the balanced chemical equations for the decomposition of solid calcium hydroxide into solid calcium (ii) oxide (lime) and
1 answer:
Calcium oxide (CaO) or lime in solid form can be prepared from the decomposition of calcium hydroxide {Ca in to lime (CaO) and water (
at high temperature. The reaction is an endothermic reaction. That is heat is absorbed in this reaction process. One mole of calcium hydroxide decomposed into one mole of calcium oxide and one mole of water. The balanced reaction can be shown as-CaC
(solid) → CaO (solid) +
(liquid). The heat of the reaction is (+) 63.7 kJ/mole of CaO.
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Answer:
The mass of HCN is 79.65 g.
The mass of reactant which remain at the end of both reactions is 88.5 g.
Explanation:
Given that,
Mass of ammonia = 50.2 g
Mass of methane = 48.4 g
Hydrogen cyanide, HCN, can be made by a two-step process
Ammonia reacts with O₂ to give nitric oxide NO.
The reaction is,
We need to calculate the mole of NO
Using given data,
2.25 g NH_{3}=\dfrac{50.2}{17}= 2.95\ mole\ NH_{3} [/tex]
2.95 mol NH₃ will produced 2.95 mol NO
Then nitric oxide reacts with methane,
The reaction is,
We need to calculate the mole of methane
Using given data,
2 mole NO produced 2 mole HCN
2.95 mol NO will produced = 2.95 mol HCN
We need to calculate the mass of HCN
Using formula of mass
Where, N = number of mole
M = molecular mass
Put the value into the formula
The mass of HCN is 79.65 g.
We need to calculate the mass of NO
Using formula of mass
Where, N = number of mole
M = molecular mass
Put the value into the formula
Hence, The mass of HCN is 79.65 g.
The mass of reactant which remain at the end of both reactions is 88.5 g.