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3 years ago

What is the nuclear binding energy of an atom that has a mass defect of 1.643 x 10-28kg?

Chemistry

2 answers:

Alla [95]3 years ago

3 0

2 (1643/200-14gk)

Will be your final answer hoped it helped

dem82 [27]3 years ago

3 0

Answer:

E = 1.4787x10^-11 J

Explanation:

To find the energy of nuclear union we must use the Einstein equation for the mass-energy equivalence, E = m*c^2, having the following data:

E = nuclear binding energy

m = mass = 1,643x10^-28 kg

c = speed of light in a vacuum = 3×10^8 m*s-1

Replacing values we have:

E = 1,643x10^-28 kg * (3x10^8 ms^-1)^2 = 1.4787x10^-11 J

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Ammonia and oxygen react to produce nitric oxide and water. Which of the following chemical equations describes this reaction an

aksik [14]

Answer:

Option B. 4NH3(g) + 5O2(g) —> 4NO(g) + 6H2O(g)

Explanation:

The reaction between ammonia, NH3 and oxygen, O2, will produce nitric oxide and water as shown below:

NH3(g) + O2(g) —> NO(g) + H2O(g)

Now, let us balance the equation.

This is illustrated below:

NH3(g) + O2(g) —> NO(g) + H2O(g)

There are 3 atoms of H on the left side and 2 atoms on the right side. It can be balance by putting 4 in front of NH3 and 6 in front of H2O as shown below:

4NH3(g) + O2(g) —> NO(g) + 6H2O(g)

There are 4 atoms of N on the left side and 1 atom on the right side. It can be balance by putting 4 in front of NO as shown below:

4NH3(g) + O2(g) —> 4NO(g) + 6H2O(g)

Now, the are 2 atoms of O on the left side and a total of 10 atoms on the right side. It can be balance by putting 5 in front of O2 as shown below:

4NH3(g) + 5O2(g) —> 4NO(g) + 6H2O(g)

Now, we can see that the equation is balanced.

Therefore, option B gives the balanced chemical equation for the reaction.

5 0

3 years ago

marishachu [46]

Answer:

B. as a food preservative in the manufacture of detergents

.........

8 0

3 years ago

fills a 500.mL flask with 3.6atm of carbon monoxide gas and 1.2atm of water vapor. When the mixture has come to equilibrium she

enot [183]

Answer:

The answer to the question is

The pressure of carbon dioxide after equilibrium is reached the second time is 0.27 atm rounded to 2 significant digits

Explanation:

To solve the question, we note that the mole ratio of the constituent is proportional to their partial pressure

At the first trial the mixture contains

3.6 atm CO

1.2 atm H₂O (g)

Total pressure = 3.6+1.2= 4.8 atm

which gives

3.36 atm CO

0.96 atm H₂O (g)

0.24 atm H₂ (g)

That is

CO+H₂O→CO(g)+H₂ (g)

therefore the mixture contained

0.24 atm CO₂ and the total pressure =

3.36+0.96+0.24+0.24 = 4.8 atm

when an extra 1.8 atm of CO is added we get Increase in the mole fraction of CO we have one mole of CO produces one mole of H₂

At equilibrium we have 0.24*0.24/(3.36*0.96) = 0.017857

adding 1.8 atm CO gives 4.46 atm hence we have

(0.24+x)(0.24+x)/(4.46-x)(0.96-x) = 0.017857

which gives x = 0.031 atm or x = -0.6183 atm

Dealing with only the positive values we have the pressure of carbon dioxide = 0.24+0.03 = 0.27 atm

7 0

3 years ago

What is the percent composition of chlorine in the compound Ba(ClO3)2?

tia_tia [17]

You're going to divide the mass of chlorine within the compound by the mass of the compound, and then multiply the result by 100 to get the answer

6 0

2 years ago

Calculate the volume in ml of 0.200 M na2co3 needed to produce 2.00 g of caco3 there is an excess of cacl2

UkoKoshka [18]

Answer:

$V=100mL$

Explanation:

Hello.

In this case, since the chemical reaction is:

$Na_2CO_3+CaCl_2\rightarrow CaCO_3+2NaCl$

We next compute the moles of sodium carbonate from the 2.00 grams of calcium carbonate via their 1:1 mole ratio in the chemical reaction:

$n_{Na_2CO_3}=2.00gCaCO_3*\frac{1molCaCO_3}{100.09gCaCO_3}*\frac{1molNa_2CO_3}{1molCaCO_3} \\\\n_{Na_2CO_3}=0.0200molNa_2CO_3$

Thus, by knowing the molarity, we compute the volume:

$M=\frac{n}{V}\\ \\V=\frac{n}{M}=\frac{0.0200mol}{0.200mol/L}\\ \\V=0.100L*\frac{1000mL}{1L}\\ \\V=100mL$

Best regards.

8 0

3 years ago