Answer:
1.429 g of N₂
Explanation:
The Haber process is a reaction that combines nitrogen with hydrogen to form ammonia according to the following balanced equation:
- N₂ ₍g₎ + 3 H₂ ₍g₎ ⇆ 2NH₃ ₍g₎
One can note that 1 mol of N₂ react with H₂ to produce 2 mol of NH₃.
We cannot compare weight of a substance (in grams) to another in chemical reactions, but we can use moles, then we have to convert the weight of NH3 to moles.
no. of moles of NH₃ = (mass / molar mass) = (1.7 g / 17 g/mol) = 0.1 mol
and the actual yield is 98% , then the theoretical number of moles that would be produced are:
- percent yield = (actual yield / theoretical yield) × 100
98 = (0.1 mol / theoretical yield) × 100
theoretical no. of moles of NH₃ = (0.1 * 100) /98 = 0.102 mol
using cross multiplication
1 mol of N₂ → 2 mol of NH₃.
?? mol of N₂ → 0.102 mol of NH₃.
no of moles of N₂ = [(1 mol * 0.102 mol) / 2 mol] = 0.051 mol
Last step is to convert the moles back to grams using:
mass = (no of moles of N₂ * molar mass of N₂)
= (0.051 mol * 28 g/mol) = 1.429 g
Non-ionizing radiation<span> does not carry enough energy to break molecular bonds and</span>ionize<span> atoms. </span>Ionizing radiation<span> is the type of </span>radiation<span> that carries enough energy to break bonds </span>between<span> molecules and </span>ionize<span> atoms.
Hope this helps!</span>
Answer:
Examples of isotones include carbon-12, nitrogen-13 and oxygen-14. These atoms all have six neutrons and six, seven and eight protons respectively. A mnemonic that can be used to differentiate isotones from isotopes and isobars is as follows: same Z (number of protons) = isotopes.
1) Reaction:
Mg(s) + 2HCl (aq) ----> H2(g) + MgCl2(aq)
2) Analysis
An increase in pressure affects directly the rate of reaction involving reactiong gases. Changing the pressure where there are only solids or liquids does not affect the rate of reaction.
This reaction is not an equilibrium, the reaction is only forward. So, the reacting components, Mg(s) and HCl(aq) are a solid and a liquid.
Therefore, the reaction is not affected by the change in pressure.
Answer: the reaction is not affected at all.
