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Anna11 [10]
3 years ago
15

In a nuclear reaction, the energy released is equal to 8.1 x 1016 joules. Calculate the mass lost in this reaction. (1 J = 1 kg

m2/s2) and the speed of light = 3.00 × 10^8 m/s ]
Answer

7.2 x 1032 kg

2.7 x 108 kg

9.0 x 10-1 kg

7.2 x 10-16 kg
Chemistry
2 answers:
makvit [3.9K]3 years ago
5 0
Use the formula E=mc^2
energy given=<span>8.1 x 10^16 joules
</span>speed of <span>light = 3.00 × 10^8 m/s
</span>
plug in the values we'll get mass=<span>9.0 x 10-1 kg</span>

N76 [4]3 years ago
3 0

Answer : The mass lost in this reaction will be, 9.0\times 10^{-1}Kg

Explanation :

According to the Einstein equation, the energy is equal to the product of mass and the square of the speed of light.

The mathematical expression is :

E=m\times c^2

where,

E = energy  released = 8.1\times 10^{16}J

c = speed of light = 3\times 10^8m/s

m = mass lost = ?

Now put all the given values in the above formula, we get the mass lost in the reaction.

8.1\times 10^{16}J=m\times (3\times 10^8m/s)^2

8.1\times 10^{16}Kg.m^2/s^2=m\times (3\times 10^8m/s)^2

m=9.0\times 10^{-1}Kg

Therefore, the mass lost in this reaction will be, 9.0\times 10^{-1}Kg

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20 ml of a solution of sucrose contains 850 mg of sucrose. What is the weight/volume percentage concentration of this solution i
MissTica
<h3>Answer:  4.25 g/ml %</h3>

Explanation:

weight/volume percentage concentration = (mass in g  ÷  volume) × 100

                                                                      =  (0.850 g ÷ 20 ml) × 100

                                                                      = 4.25 g/ml %

∴ the weight/volume percentage concentration of the sucrose solution is 4.25 g/ml %.

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A compound with a molar mass of 60g/mol is 40.4% carbon, 6.7% hydrogen and 53.3% oxygen (by mass). determine the emperical and m
Fittoniya [83]

<span>A compound is found to be 40.0% carbon, 6.7% hydrogen and 53.5% oxygen. Its molecular mass is 60. g/mol. 
</span>Q1)
Empirical formula is the simplest ratio of whole numbers of components making up a compound.
the percentages have been given, therefore we can calculate for 100 g of the compound.

                                C                            H                        O
Mass in 100 g      40.0 g                       6.7 g                   53.5 g
Molar mass            12 g/mol                1 g/mol                 16 g/mol
Number of moles   40.0/12= 3.33         6.7/1 = 6.7          53.5/16 = 3.34
Divide by the least number of moles  
                             3.33/3.33 = 1           6.7/3.33 = 2.01   3.34/3.33 = 1.00
after rounding off
C - 1 
H - 2
O - 1

Empirical formula - CH₂O

Q2)
Molecular formula is the actual number of components making up the compound.
To find the number of empirical units we have to find the mass of one empirical unit.
Mass of one empirical unit = CH₂O - 12 + (1x2) + 16 = 30 g
Mass of one mole of compound = 60 g
Number of empirical units = 60 g / 30 g = 2
Therefore molecular formula - 2(CH₂O) 
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Arlecino [84]

Answer:

Explanation:

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