Answer: E
How much NH₃ can be produced from the reaction below:
N₂ + 3H₂ - 2NH₃
The stoichiometric ratio of the reactants = 1:3
Given
74.2g of N₂, and Molar mass = 14g/mole
Mole of N₂ = 74.2/14=5.3mols of N₂,
and 14mols of H₂
From this given values and comparing with the stoichiometric ratio, H₂ will be the limiting reagent while N₂ is the excess reactant.
i.e, for every 14mols of H₂, we need 4.67mols of N₂ to react with it to produce 9.33mols of NH₃ as shown (vice versa)
From this we have 9.33mols of NH₃ produced
Avogadro constant, we have n = no of particles = 6.022x10²³ molecules contained in every mole of an element.
For a 9.33mols of NH3, we have 9.33x6.022x10²³molecules in NH3
5.62x10²⁴molecules of NH₃
False is the correct answer.
A higher concentration of reactants leads to more collisions per unit time and leads to an increasing reaction rate. Changing the pressure of gaseous reactants is, in effect, changing their concentration. The increased number of collisions caused by a higher pressure generally increases the reaction rate.
Potato cells contains starch. When you add iodine solution into potato cells, you may observe that the brown color of iodine on the potato changes into a blue black color. This is because a starch/iodine complex is formed and it has a blue black color.
Answer:
Ca + AgNO3 ---> Ca(NO3)2 + Ag
Calcium + silver nitrate ---> Calcium nitrate + silver
also ...reaction type is Single displacement reaction .
hope this answer's your question.
