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fredd [130]
2 years ago
13

How many grams of oxygen can be obtained from 250. grams of KCIO3?

Chemistry
1 answer:
guapka [62]2 years ago
3 0

Answer:

Keep it simple. If all the oxygen contained in the 200 grams of potassium chlorate is produced in the decomposition, then all we have to do is find out how many grams of oxygen are there in the 200 grams. This we can do by calculating the ratio of oxygen mass to the whole. Using 39.1 for potassium, 35.45 for chlorine and 3 times 16, or 48 for the oxygen, we get a total of 122.55 grams per mole for potassium chlorate, of which 48 grams are oxygen. This ratio is 48/122.55. This ratio times the original 200 grams of the compound, gives us 78.34 grams of oxygen produced.

Explanation:

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Anemia is essentially an iron deficiency so the element found in the liver preventing it would be Fe (iron).
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How many moles of aluminum are needed to make 9 moles of molecular hydrogen? Given the reaction: 2 Al + 6 HCl → 2 AlCl3 + 3H2
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Answer:

We need 6.0 moles of aluminium

Explanation:

Step 1: Data given

Number of moles of H2 = 9.0 moles

Step 2: The balanced equation

2 Al + 6 HCl → 2 AlCl3 + 3H2

Step 3: Calculate moles Al

For 2 moles Aluminium, we need 6 moles HCl to produce 2 moles AlCl3 and 3 moles H2

For 9.0 moles of H2 we need 2/3 * 9.0 = 6.0 moles of aluminium

We need 6.0 moles of aluminium

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Need help with 14 and 16 pls asap!! this is my friends test and im taking it tomorrow!!
marin [14]

Answer:

Q14: 17,140 g = 17.14 kg.

Q16: 504 J.

Explanation:

<u><em>Q14:</em></u>

  • To solve this problem, we can use the relation:

<em>Q = m.c.ΔT,</em>

where, Q is the amount of heat absorbed by ice (Q = 3600 x 10³ J).

m is the mass of the ice (m = ??? g).

c is the specific heat of the ice (c of ice = 2.1 J/g.°C).

ΔT is the difference between the initial and final temperature (ΔT = final T - initial T = 100.0°C - 0.0°C = 100.0°C).

∵ Q = m.c.ΔT

∴ (3600 x 10³ J) = m.(2.1 J/g.°C).(100.0°C)

∴ m = (3600 x 10³ J)/(2.1 J/g.°C).(100.0°C) = 17,140 g = 17.14 kg.

<u><em>Q16:</em></u>

  • To solve this problem, we can use the relation:

<em>Q = m.c.ΔT,</em>

where, Q is the amount of heat absorbed by ice (Q = ??? J).

m is the mass of the ice (m = 12.0 g).

c is the specific heat of the ice (c of ice = 2.1 J/g.°C).

ΔT is the difference between the initial and final temperature (ΔT = final T - initial T = 0.0°C - (-20.0°C) = 20.0°C).

∴ Q = m.c.ΔT = (12.0 g)(2.1 J/g.°C)(20.0°C) = 504 J.

6 0
2 years ago
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