8. (02.04 MC)
1 answer:
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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:
Gas X
Explanation:
The given reaction can be written in the form of chemical equation as shown below as:
According to law of conservation of mass, the moles of each substance in the reaction must be equal on both reactant and product side.
Also, the question asks for the gas which is diatomic. cannot be diatomic as the formula contains 3 atoms.
Between gas X and gas Y , <u>X has to be diatomic for the reaction to balance </u>as: