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Rudik [331]
3 years ago
11

In a nuclear reaction, the energy released is equal to 5.4 x 1015 joules. Calculate the mass lost in this reaction. (1 J = 1 kg

m2/s2)
6.0 x 10-2 kg
4.86 x 10-1 kg
1.8 x 10-1 kg
1.62 x 102 kg
Chemistry
2 answers:
Alexeev081 [22]3 years ago
3 0
I think the answer is A.
FinnZ [79.3K]3 years ago
3 0

Answer:

A) 6 *10^-2 kg

Explanation:

From Einstein equation of mass and energy inter conversion,

E = MC²

E = Energy released = 5.4 * 10¹⁵ J

M = mass = ?

C = spend of light = 3.0*10⁸m / s

E = mc²

M = E / c²

M = 5.4 * 10¹⁵ / (3.0 * 10⁸)²

M = 0.06kg = 6 * 10^-2 kg

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Hii pls help me!! <br>even if u know how to do one, it's okk <br>anything helps ​
tensa zangetsu [6.8K]

Explanation:

a) HNO2(aq) = HNO3(aq) + H2O(l) +NO(g)

b) SoCl2 (l) + H2O (l) = So2(g) + 2HCl(aq)

c) CH4 (g) + 2O2(g) = Co2 (g) + 2H2O(g)

d) 3CuO(s) + 2NH3 (g) = 3Cu(s) + 3H2O (l) + N2(g)

3 0
3 years ago
What is the difference between atomic mass, relative atomic mass and average atomic mass
vesna_86 [32]

\bold{\huge{\underline{\purple{ Answer }}}}

<u>Difference </u><u>between </u><u>Atomic </u><u>mass</u><u>, </u><u>relative </u><u>atomic </u><u>mass </u><u>and </u><u>average </u><u>atomic </u><u>mass</u><u> </u><u>:</u><u>-</u>

<h3><u>Atomic </u><u>Mass </u><u>:</u><u>-</u></h3>

  • Atomic mass is the mass of neutrons and protons present in the nucleus of an atom .
  • It is always calculated for a single element and having direct value
  • For isotopes also, the atomic mass is calculated separately . Example :- <u>Carbon </u><u>1</u><u>2</u><u> </u><u>,</u><u> </u><u>carbon </u><u>1</u><u>3</u><u> </u><u>and </u><u>carbon </u><u>1</u><u>4</u><u> </u><u>have </u><u>different </u><u>atomic </u><u>mass</u><u>. </u>
  • The SI unit of Atomic mass is " u" and "amu"

<h3><u>Relative </u><u>Atomic </u><u>mass </u><u>:</u><u>-</u></h3>

  • Relative atomic mass is mean mass of the atoms of an element which is compared to the 1/12th mass of carbon - 12 .
  • Carbon - 12 is taken as a relative when we calculate the relative atomic mass of any element
  • For calculating relative atomic mass, we need to know the masses, percentage and abundance of all types of elements
  • Relative atomic mass is a dimension less quantity

<h3><u>Average </u><u>Atomic </u><u>Mass </u><u>:</u><u>-</u></h3>

  • Average atomic mass is the average mass of an atoms of a particular element by considering it's isotopes
  • While we calculate average atomic mass is a standardized number. Whereas, Average atomic mass sometimes varies geologically .
  • It also includes percentage, abundance and masses of given element .
  • In average atomic mass, We do not compare mean value with the 1/12 mass of carbon - 12
  • The unit of Average atomic mass is "Amu" or " u " .
5 0
2 years ago
The dissolution of 0.200 l of sulfur dioxide at 19 °c and 745 mmhg in water yields 500.0 ml of aqueous sulfurous acid. The solut
aivan3 [116]

Answer:

Molarity=1.22\ M

Explanation:

Given:  

Pressure = 745 mm Hg

Also, P (mm Hg) = P (atm) / 760

Pressure = 745 / 760 = 0.9803 atm

Temperature = 19 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = (19 + 273.15) K = 292.15 K  

Volume = 0.200 L

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.9803 atm × 0.200 L = n × 0.0821 L.atm/K.mol × 292.15 K  

⇒n = 0.008174 moles

From the reaction shown below:-

H_2SO_3+2NaOH\rightarrow Na_2SO_3+2H_2O

1 mole of H_2SO_4 react with 2 moles of NaOH

0.008174 mole of H_2SO_4 react with 2*0.008174 moles of NaOH

Moles of NaOH = 0.016348 moles

Volume = 13.4 mL = 0.0134 L ( 1 mL = 0.001 L)

So,

Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}

Molarity=\frac{0.016348}{0.0134}\ M

Molarity=1.22\ M

8 0
3 years ago
I NEED HELP PLEASE!!!! CHEMISTRY QUESTION: If 38 g of Li3P and 15 grams of Al2O3 are reacted, what total mass of products will r
maksim [4K]

Answer:

21.5 g.

Explanation:

Hello!

In this case, since the reaction between the given compounds is:

2Li_3P+Al_2O_3\rightarrow 3Li_2O+2AlP

We can see that according to the law of conservation of mass, which states that matter is neither created nor destroyed during a chemical reaction, the total mass of products equals the total mass of reactants based on the stoichiometric proportions; in such a way, we first need to compute the reacted moles of Li3P as shown below:

n_{Li_3P}^{reacted}=38gLi_3P*\frac{1molLi_3P}{51.8gLi_3P}=0.73molLi_3P

Now, the moles of Li3P consumed by 15 g of Al2O3:

n_{Li_3P}^{consumed \ by \ Al_2O_3}=15gAl_2O_3*\frac{1molAl_2O_3}{101.96gAl_2O_3} *\frac{2molLi_3P}{1molAl_2O_3} =0.29molLi_3P

Thus, we infer that just 0.29 moles of 0.73 react to form products; which means that the mass of formed products is:

m_{Li_2O}=0.29molLi_3P*\frac{3molLi_2O}{2molLi_3P} *\frac{29.88gLi_2O}{1molLi_2O} =13gLi_2O\\\\m_{AlP}=0.29molLi_3P*\frac{2molAlP}{2molLi_3P} *\frac{57.95gAlP}{1molAlP} =8.5gAlP

Therefore, the total mass of products is:

m_{products}=13g+8.5g\\\\m_{products}=21.5g

Which is not the same to the reactants (53 g) because there is an excess of Li₃P.

Best Regards!

7 0
3 years ago
Determine the name of the compound Li2O
eduard
Lithium Oxide
I just search it up to be honest
7 0
3 years ago
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