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Fiesta28 [93]
3 years ago
11

A 5 kg block

Chemistry
1 answer:
Burka [1]3 years ago
4 0

Answer:

By Newton's 2nd law, m*a=sum_of_forces where m is the mass and a the acceleration. Here there are two forces in opposed directions.

Thus 5*a=40-8=32 therefore a=32/5=6.4m^s/2

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Ignore this!<br><br>i got the answer already haha
marta [7]

Answer:

okay lol, ima use this for points if okay

Explanation:

5 0
3 years ago
what mass of aluminium hydroxide is needed to decompose in order to produce 65.0 L of water at STP in stoichiometry?
pishuonlain [190]
Aluminium Hydroxide on decomposition produces Al₂O₃ and Water vapors. 

<span>                               2 Al(OH)</span>₃    →    Al₂O₃  +  3 H₂O


According to equation at STP,

       67.2 L (3 moles) of H₂O is produced by  =  78 g of Al(OH)₃
So,
                65.0 L of H₂O will be produced by  =  X g of Al(OH)₃

Solving for X,
                                 X  =  (65.0 L × 78 g) ÷ 67.2 L

                                 X  =  75.44 g of Al(OH)₂
Result:
           75.44 g of Al(OH)₂ is needed to decompose in order to produce 65.0 L of water at STP in stoichiometry
6 0
2 years ago
Read 2 more answers
What does FE stand for in the Periodic Table of Elements?
sveticcg [70]
It stabds for Iron.
6 0
3 years ago
Read 2 more answers
For the first-order reaction, 2 n2o(g) → 2 n2(g) + o2(g), what is the concentration of n2o after 3 half-lives if 0.25 mol of n2o
g100num [7]
According to that each half-life we lose half of the concentration of N2O so,

Because we start with a concentration of N2O = 0.25 mol 
so after one half-life the concentration of N2O decrease to the half 0.25/2
= 12.5 x 10^-2 M
and after two half-lives the concentration of N2O of the one half-life decrease to the half (12.5 x 10^-2) / 2 
=6.25 x 10^-2 M
and after three half-lives the concentration of N2O of the two half-lives decrease to the half (6.25x10^-2) / 2
= 3.1 x 10^-2 M
∴ your correct answer is 3.1 x 10^-2 M
6 0
3 years ago
Read 2 more answers
Given:
Solnce55 [7]

Answer:

113.4g of N2

Explanation:

Step 1:

The balanced equation for the reaction.

N2 + 3H2 —> 2NH3

Step 2:

Determination of the mass of N2 and H2 that reacted from the balanced equation. This is illustrated below:

Molar mass of N2 = 2x14 = 28g/mol

Mass of N2 from the balanced equation = 1 x 28 = 28g

Molar mass of H2 = 2x1 = 2g/mol

Mass of H2 from the balanced equation = 3 x 2 = 6g

From the balanced equation above, 28g of N2 reacted with 6g of H2.

Step 3:

Determination of the mass N2 required to react with 24.3g of H2.

The mass of N2 required to react with 24.3g of H2 can be obtained as follow:

From the balanced equation above, 28g of N2 reacted with 6g of H2.

Therefore, Xg of N2 will react 24.3g of H2 i.e

Xg of N2 = (28 x 24.3)/6

Xg of N2 = 113.4g

Therefore, 113.4g of N2 is required to react completely with 24.3g of H2.

7 0
3 years ago
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