Consider the reaction N2(g) + 3H2(g) → 2NH3(g) Suppose that at a particular moment during the reaction, molecular hydrogen is reacting at the rate of −0.091 M/s.
(a) At what rate is ammonia being formed? M/s
(b) At what rate is molecular nitrogen consumed? M/s

The solution to the question is as follows

(a) The rate of ammonia formation = 0.061 M/s

(b) the rate of N₂ consumption = 0.0303 M/s

Explanation:

(a) To solve the question we note that the reaction consists of one mole of N₂ combining with three moles of H₂ to form 2 moles of NH₃

N₂(g) + 3H₂(g) → 2NH₃(g)

The rate of reaction of molecular hydrogen = 0.091 M/s, hence we have

3 moles of H₂ reacts to form 2 moles of NH₃, therefore

0.091 M of H₂ will react to form 2/3 × 0.091 M or 0.061 M of NH₃

Hence the rate of ammonia formation is 0.061 M/s

(b) From the reaction equation we have 3 moles of H₂ and one mole of N₂ being consumed at the same time hence

0.091 M of H₂ is consumed simultaneously with 1/3 × 0.091 M or 0.0303 M of N₂

Therefore the rate of consumption of N₂ = 0.0303 M/s

a. they must be certified by the avma.

explanation:

mark brainliest and have a great day!

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.