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denis23 [38]
2 years ago
7

5. How many grams of potassium bromide will dissolve in 450g of water at 80°C?

Chemistry
1 answer:
Shtirlitz [24]2 years ago
6 0
Hi mate. I think the answer is 100
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In the equation:<br><br> 23491Pa → 234 92U + X<br><br><br> The X represents a
Bad White [126]
Beta particle in the reaction
3 0
3 years ago
Determine whether each of the following statements about sulfur oxide and/or nitrogen oxide pollution is true or false.
astraxan [27]

Answer:

a) False

b) False

c) True

Explanation:

a) Most sulfur oxides formed during combustion come from sulfur in the air: The sulfur burns in presence of oxygen to produce sulfur oxides, the source of sulfur is anthropogenic activities (Human activities).

So the given statement is false.

b) A flue gas scrubber removes SO2 pollution in a coal-fired power plant by using lime to convert the SO2 into alcohols:

False

The lime reacts with sulfur dioxide to give carbon dioxide and calcium sulfite.

CaCO_{3}+SO_{2}--->CaSO_{3}+CO_{2}

c) True

c)

3 0
2 years ago
During studies of the following reaction (i), a chemical engineer measured a less-than-expected yield of N2 and discovered that
bonufazy [111]

Answer:

Maximum expected yield = 87.2%

Explanation:

Equations of reactions:

Main reaction: N₂O₄(l) + 2N₂H₄(l) ---> 3N₂(g) + 4H₂O(g)

Side reaction:  2N₂O₄(l) + N₂H₄(l) ----> 6NO(g) + 2H₂O(g)

Molar mass of N₂O₄ = 92 g/mol; molar mass of N₂H₄ = 32 g/mol; molar mass of N₂ = 28 g/mol; molar mass of of NO = 30 g/mol; molar mass of water = 18 g/mol

In the main reaction, 92 g of N₂O₄ reacts with 2 * 32 g of N₂H₄ to produce 3 * 14 g of N₂.

101.1 g of N₂O₄ will react with 2 * 32 * 101.1 / 92 g of N₂H₄ = 70.33 g of N₂H₄

<em>N₂O₄ is the limiting reactant</em>

101.1 g of N₂O₄ will react to produce 3 * 14 * 101.1 / 92 g of N₂ =  46.15 g of  N₂

In the side reaction, (6 * 30 g) of NO  is produced  from (2 * 92 g) of N₂O₄ and 32 g of N₂H₄

12.7 g of N₂O₄ will be produced from ( 2 * 92 * 12.7/180 g) of N₂O₄ and (32 * 12.7/180) g of N₂H₄ to produce

mass of N₂O₄ used = 12.98 g

mass of N₂H₄ used = 2.26 g

mass of N₂O₄ left for main reaction = 101.1 - 12.98 = 88.12 g

mass of N₂H₄ left for main reaction = 101.1 - 2.26 = 98.84 g

In the main reaction, 92 g of N₂O₄ reacts with 2 * 32 g of N₂H₄ to produce 3 * 14 g of N₂

88.12 g of N₂O₄ will react with 2 * 32 * 88.12 / 92 g of N₂H₄ = 61.30 g of N₂H₄

N₂O₄ is the limiting reactant.

88.12 g of N₂O₄ will to react produce 3 * 14 * 88.12 / 92 g of N₂ =  40.23 g of  N₂

Percentage yield = (theoretical yield/actual yield) * 100%

Percentage yield = (40.23/46.15) * 100% = 87.2%

Therefore, maximum expected yield = 87.2%

4 0
2 years ago
Hands on mole activity
Amanda [17]

Explanation:

one mole= 6.02x10^23

Everything going from a mole will always be multiplied and everything going into mole will be divided.

4 0
3 years ago
You are working out on the treadmill machine at the gym. The machine says that you are burning 110 calories per mile (110 calori
RoseWind [281]

So 500/110=4.54545455, so 4.54545455 rounded to the nearest hundredth is 4.55 miles!

5 0
2 years ago
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