Answer:
Spontaneous and random. Decay is called spontaneous because the occur on their own and are unaffected by external factors like temperature, pressure, and many more. Decay is called random because we cannot determine the rate at which it decays but can only determine the probability of the decay.Oct 21, 2015
Explanation:
Both trials of 1.2 g and 1.6 g will have the same mass percent of water because the ratio of the salt to the water of hydration is always constant for any hydrated salt.
<h3>Water of hydration</h3>
For every hydrated salt, the ratio of the salt to the water of hydration remains constant irrespective of the amount of salt taken for experimental analysis.
For example, assuming the mass percent of water in 10g of a hydrated salt is 40%, if 100g of the same salt is taken, the mass percent will remain 40%.
More on water of hydration can be found here: brainly.com/question/11202174
Answer:
It donates a hydrogen ion
Explanation:
Under the Bronsted-Lowry definition of an acid, acids are protons donors which donate the H+ ion, or the hydrogen ion.
Answer:
Oxidation by FAD
Explanation:
1. Oxidation by NAD⁺
Succinate ⇌ Fumarate + <u>2H⁺ + 2e⁻</u>; E°´ = -0.031 V
<u>NAD⁺ + </u><u>2H⁺ + 2e⁻</u><u> ⇌ NADH + H⁺; </u> E°´ = <u> -0.320 V</u>
Succinate + NAD⁺ ⇌ Fumarate + NADH + H⁺; E°' = -0.351 V
2. Oxidation by FAD
Succinate ⇌ Fumarate + 2H⁺ + 2e⁻; E°´ = -0.031 V
<u>FAD + 2H⁺ + 2e⁻ ⇌ FADH₂; </u> E°´ = <u>-0.219 V
</u>
Succinate + FADH₂ ⇌ Fumarate + FAD; E°' = -0.250 V
Neither reaction is energetically favourable, but FAD has a more positive half-cell potential.
FAD is the stronger oxidizing agent.
The oxidation by FAD has a more positive cell potential, so it is more favourable energetically.
Answer:
The answer to your question is 68.8%
Explanation:
Data
Iron = 3.8 moles
Sulfur = excess
FeS = 230 g
Molecular weight FeS = 88 g
Process
Reaction
Fe + S ⇒ FeS
1.- Convert the number of moles of Iron to grams
56 g of Iron -------------- 1 mol
x -------------- 3.8 moles
x = (3.8 x 56) / 1
x = 212.8 g of Iron
2.- Calculate the theoretical production of FeS
56 g of Iron ---------------- 88 g of FeS
212.8 g of iron ----------- x
x = (212.8 x 88) / 56
x = 334.4 g of FeS
3.- Calculate the percent yield
% yield = 
% yield = 68.8
