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Zolol [24]
3 years ago
10

A quantity of energy equal to 8.90 × 1012 joules was emitted from a nuclear reaction. What amount of mass was required to be con

verted to yield this amount of energy?
9.90 × 10-5 kg

2.96 × 10-4 kg

2.67 × 104 kg

8.01 × 105 kg
Chemistry
2 answers:
LenKa [72]3 years ago
6 0

Answer : The amount of mass required will be, 9.90\times 10^{-5}Kg

Explanation :

The formula used for energy is :

E=m\times c^2

where,

E = energy = 8.90\times 10^{12}J

m = mass = ?

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

Now put all the given values in this formula, we get :

8.90\times 10^{12}J=m\times (3\times 10^8m/s)^2

m=9.90\times 10^{-5}Kg

Therefore, the amount of mass required will be, 9.90\times 10^{-5}Kg

Nataly [62]3 years ago
5 0
E = mc^2
E = 8.90 * 10^12 Joules
c = 3 * 10^8 m/s
m = ????

8.90 * 10^12 = m * (3 * 10^8)^2
8.90 * 10^12 = m * 9 * 10^16
9.889 * 10^-4 kg = m <<<<< answer
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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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What is the total ionic equation for the following reaction?
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Explanation:

An equation in which electrolytes are represented in the form of ions is known as an ionic equation.

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Help! What did I do wrong??
iogann1982 [59]

The molecules  of hydrogen gas that are  formed is  when 48.7 g  of sodium are added to water  is  6.375  x 10²³  molecules


  <u><em>calculation</em></u>

2 Na +2H₂O →  2 NaOH  +H₂

Step 1: find the moles  of sodium (Na)

moles =mass÷   molar mass

from periodic table the molar mass of Na = 23 g/mol

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Step 2:use the mole ratio to determine  the  moles of H₂

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therefore the moles  of H₂ = 2.117 moles x 1/2=1.059 moles

Step 3: find the molecules of H₂ using the Avogadro's law

According  to  Avogadro's  law  1 mole = 6.02 x 10²³ molecules

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by cross multiplication

= [(1.059 moles x 6.02 x10²³  molecules) /  1 mole] =6.375  x 10²³  molecules

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