The mass of sulfur in a sample of CaSO4 with a mass of 65.8 g is 15.50g.
<h3>How to calculate mass of an element in a compound?</h3>
According to this question, a 10.4 g sample of CaSO4 is found to contain 3.06 g of Ca and 4.89 g of O.
This means that the mass of sulfur in the 10.4g of CaSO4 is 10.4g - (3.06g + 4.89g) = 10.4g - 7.95g = 2.45g
Next, we calculate the percent ratio of each element in the compound; CaSO4.
- Ca = 3.06g/10.4g × 100 = 29.42%
- S = 2.45g/10.4g × 100 = 23.56%
- O = 4.89g/10.4g × 100 = 47.02%
According to this question, a sample of CaSO4 with a mass of 65.8 g is given. The mass of each element in this compound is as follows:
- Ca = 29.42/100 × 65.8g = 19.36g
- S = 23.56/100 × 65.8g = 15.50g
- O = 47.02/100 × 65.8g = 30.94g
Therefore, the mass of sulfur in a sample of CaSO4 with a mass of 65.8 g is 15.50g.
Learn more about mass at: brainly.com/question/13672279
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Answer: the mass number of an element is equal to the number of protons plus the number of neutrons.
Such high amounts of pressure cause this layer to remain in a _____solid_____ state of matter even though the nickel and iron are at such a high temperature.
Answer:
0.0253 M/s
Explanation:
From the reaction
N₂ + 3H₂ → 2NH₃
The rate of reaction can be written as
Rate = - ![\frac{d[N_2]}{dt}](https://tex.z-dn.net/?f=%5Cfrac%7Bd%5BN_2%5D%7D%7Bdt%7D)
= - ![\frac{1}{3} \frac{d[H_2]}{dt}](https://tex.z-dn.net/?f=%5Cfrac%7B1%7D%7B3%7D%20%5Cfrac%7Bd%5BH_2%5D%7D%7Bdt%7D)
= + ![\frac{1}{2} \frac{d[NH_3]}{dt}](https://tex.z-dn.net/?f=%5Cfrac%7B1%7D%7B2%7D%20%5Cfrac%7Bd%5BNH_3%5D%7D%7Bdt%7D)
From the above rate equation we can conclude that the rate of reaction of N₂ is equal to one third of the rate of reaction of H₂,
So,
Rate of reaction of molecular nitrogen = 
Upon calculation, we get rate of reaction of molecular nitrogen = 0.0253 M/s
