Aqueous hydrogen chloride reacts with oxygen gas to form chlorine gas and liquid water.Express your answer as a balanced chemica
2 answers:
4HCl (aq) + O₂ (g) ⇒ 2Cl₂ (g) + 2H₂O (l)
<h3>Further explanation </h3>Equalization of chemical reactions can be done using variables. Steps in equalizing the reaction equation:
- 1. gives a coefficient on substances involved in the equation of reaction such as a, b, or c, etc.
- 2. make an equation based on the similarity of the number of atoms where the number of atoms = coefficient × index (subscript) between reactant and product
- 3. Select the coefficient of the substance with the most complex chemical formula equal to 1
For gas combustion reaction which is a reaction of hydrocarbons with oxygen produces CO₂ and H₂O (water vapor). can use steps:
Balancing C, H and the last O
Reaction :
HCl (aq) + O₂ (g) ⇒ Cl₂ (g) + H₂O (l)
Suppose we give a coefficient of 1 for HCl
HCl (aq) + aO₂ (g) ⇒ bCl₂ (g) + cH₂O (l)
number of Homs: left 1, right 2c -> 2c = 1-> c = 1/2
number of Cloms: left 1, right 2b ---> 2b = 1 ----> b = 1/2
number of O atoms: left 2a, right c ---> 2a = c ---> 2a = 1/2 ---> a = 1/4
the reaction coefficient becomes:
the combustion of octane in gasoline
hydrogen and excess oxygen
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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.
Answer:
a) 2KOH + NiSO₄ → K₂SO₄ + Ni(OH)₂
b) Ni(OH)₂
c) KOH
d) 0.927 g
e) K⁺=0.067 M, SO₄²⁻=0.1 M, Ni²⁺=0.067 M
Explanation:
a) The equation is:
2KOH + NiSO₄ → K₂SO₄ + Ni(OH)₂ (1)
b) The precipitate formed is Ni(OH)₂
c) The limiting reactant is:
From equation (1) we have that 2 moles of KOH react with 1 mol of NiSO₄, so the number of moles of KOH is:
Hence, the limiting reactant is KOH.
d) The mass of the precipitate formed is:
e) The concentration of the SO₄²⁻, K⁺, and Ni²⁺ ions are:
I hope it helps you!