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ivolga24 [154]
3 years ago
11

The compound mgso4, epsom salts, is used to soothe sore feet and muscles. how many grams will you need to prepare a bath contain

ing 5.40 mol of epsom salts?
Chemistry
2 answers:
VLD [36.1K]3 years ago
8 0

Answer: Mass= n x molar mass= 4.00 moles x 120.4 g/mol = 482 g

Explanation:

number of moles = mass/ molar mass

Gala2k [10]3 years ago
3 0

Answer:

648 grams of epsom salt will be needed.

Explanation:

Mass of magnesium atom = 24  g/mol

Mass of sulfur atom= 32 g/mol

Mass of oxygen atom= 16 g/mol

Molar mass of epsom salt: 24 g/mol+32 g/mol+4\times 16 g/mol=120 g/mol

Moles of epsom salt in water = 5.40 mol

Mass of 5.40 moles of  epsom salt : Molar mass × Moles:

=120 g/mol\times 5.40 mol=648 g

648 grams of epsom salt will be needed.

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How do I calculate the sum of 6.078 g and 0.3329 g ?
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The answer is 6.4109 grams
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Identify the oxidizing and reducing agents in the following: H2S(aq) + Cl2(g) -> S(s) + 2HCI (aq)
alexgriva [62]

The oxidizing and reducing agent in the above redox reaction are hydrogen sulphide (H2S) and Chlorine (Cl) respectively.

<h3>What is an oxidizing and reducing agent?</h3>

An oxidizing agent is any substance that oxidizes, or receives electrons from another substance and as a result, becoming reduced.

On the other hand, a reducing agent is any substance that reduces or donates electrons to another and as a result becomes oxidized.

According to this reaction; H2S(aq) + Cl2(g) -> S(s) + 2HCI (aq)

  • H2S accepts electrons from Cl2 and becomes reduced to S
  • Cl2 donates electrons to H2S and becomes oxidized to HCl

Therefore, the oxidizing and reducing agent in the above redox reaction are hydrogen sulphide (H2S) and Chlorine (Cl) respectively.

Learn more about oxidizing agent at: brainly.com/question/10547418

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8 0
1 year ago
A student weighs out 0. 0422 g of magnesium metal. The magnesium metal is reacted with excess hydrochloric acid to produce hydro
lutik1710 [3]
  • The student weighs out 0.0422 grams of the metal magnesium, thus we can figure that the more's, the magnesium he used, is the mass of the magnesium over the more mass, which is 0.024422.
  • That is approximately 0.001758.
  • Furthermore, it claims that too much hydrochloric acid causes the metal magnesium to react, producing hydrogen gas.
  • The volume of collected gas is 43.9 cc, the mastic pressure is 22 cc, and a sample of hydrogen gas is collected over water in a meter.
<h3>Is it true that calculations made utilizing experimental and gathered data result in a percent error? </h3>
  • Consequently, we are aware that magnesium and chloride react.
  • We create 1 as the reaction ratio is 1:2.
  • The hydrogen and 1 are more.
  • Magnesium chloride is more.
  • Therefore, based on this equation, we can infer that the amount of hydrogen that would be created in this scenario is greater than the amount of magnesium present here, or 0.001758 more.
  • Among hydrogen, there is.
  • \Once we convert the temperature from 32 Celsius to kelvin, we can tell you that the temperature is actually about 5.15 kelvin.
  • The gas has a volume of 43 in m, which is equal to 0.0439 liter and indicates that the pressure is approximately 832 millimeter.
  • Mercury, which is 2 times 13332 plus ca, or roughly 110922.24 par, is a mathematical constant.
  • So, in this instance, we are aware that p v = n r t.
  • The r in this case equals p v over n t, thus we want to determine the r.
  • So p is 110922.24. The temperature is 305.15 and the V is 0.04  over the n is 0.001758.
  • Let's proceed with the calculations right now.
  • In this instance, you will discover that the solution is 9.077 times 10; that is all there is to it.

To learn more about Magnesium chloride reactions visit:

brainly.com/question/27891157

#SPJ4

3 0
2 years ago
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