Hydrogen gas and nitrogen gas react to form ammonia gas. What volume of ammonia would be produced by this reaction if of nitroge
1 answer:
Answer:
1.38*10^4 L or 0.138*10^2 m^3
Explanation:
The balanced equation for the reaction is:
⇒
In the chemical equation above, 3 moles of hydrogen gas react with 1 mole of nitrogen gas to produce 2 moles of ammonia gas. A STP, 1 mole of gas is equivalent to 22.4 L. Therefore,
6.9 m^3 of nitrogen gas will be equivalent to 6900 L. In addition, 6900L will be equivalent to 6900/22.4 = 308.036 moles
1 mole of nitrogen produced 2 moles of ammonia gas, therefore, 308.04 moles of nitrogen gas would produce 2*308.036 moles = 616.07 moles of ammonia gas
At STP, 1 mole of gas is equivalent to 22.4 L, thus 616.07 moles will be equivalent to 22.4*616.07 = 13800 L or 13.8 m^3
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Answer: The volume of required is 25.0 ml
Explanation:
According to the neutralization law,
where,
= basicity
= 1
= molarity of
solution = 2.00 M
= volume of
solution = 50.0 ml
= acidity of
= 1
= molarity of
solution = 4.00 M
= volume of
solution = ?
Putting in the values we get:
Therefore, volume of required is 25.0 ml
Answer:
0.6g
Explanation:
Given parameters:
Mass of K = 0.5g
Mass of O₂ = 0.10g
Unknown:
Mass of K₂O = ?
Solution:
To solve this problem, let us write the reaction equation first;
4K + O₂ → 2K₂O
The reaction above delineates the balanced chemical reaction.
To solve this problem, we need to know the limiting reactant. This reactant is the one that determines the amount and extent of the reaction because it is given in short supply. The other reactant is the one in excess.
Start off by find the number of moles of the reactant;
Number of moles =
Molar mas of K = 39g/mol
Molar mass of O₂ = 2(16) = 32g/mol
Number of moles of K = = 0.013moles
Number of moles of O₂ = = 0.031moles
From the balanced reaction;
4 moles of K reacted with 1 mole of O₂
0.013 moles of K will react with = 0.0078 moles of O₂
We see that oxygen gas is in excess. We were given 0.031moles of the gas but only require 0.0078moles of oxygen gas.
The limiting reactant is potassium.
therefore;
4 moles of K produced 2 moles of K₂O
0.013 moles of K will produce = 0.0065moles of K₂O
to find the mass of K₂O;
Mass of K₂O = number of moles x molar mass
Molar mass of K₂O = 2(39) + 16 = 94g/mol
Mass of K₂O = 0.0065 x 94 = 0.6g
Answer:
C. No, because the carbon chain is composed of only a single ring.
Polycyclicity, having more than a single ring, is a property of only aromatic hydrocarbons. Therefore, if the hydrocarbon is not polycyclic, it is non-aromatic
Explanation:
Cyclic Hydrocarbons
These are organic compounds which are cyclic in structure. The compound cyclohexane involves a ring of six carbon atoms, each of which is also bonded to two hydrogen atoms
Aromatic hydrocarbons are cyclic ring organic compound which are based on the benzene ring structure.
A. If the hexagon contains single bonds, it is non-aromatic.
B. No. Having a ring shape does not on its own determine the aromaticity of a hydrocarbon.
C. Polycyclicity, having more than a single ring, is a property of only aromatic hydrocarbons. Therefore, if the hydrocarbon is not polycyclic, it is non-aromatic
D. Having double bonds within a ring is not a criteria for being aromatic. Both aromatic and non-aromatic hydrocarbons have double bonds within their rings. However, aromatic hydrocarbons have alternate double and single bonds within their 6-carbon ring structure.
Note: Since the structure of the required hydrocarbon is not shown, the explanation contains attachments of hexagonal structures of three hydrocarbons; one non-aromatic and the other two are aromatic. Cyclohexane is non-aromatic while Benzene and the polycyclic compounds are aromatic.
