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Natali [406]
3 years ago
5

Are nuclear bombs ethical? Explain please

Chemistry
2 answers:
Mrac [35]3 years ago
6 0

Answer:

<u>Yes, they are.</u>

Explanation:

The United States is one of these nuclear superpowers, making the ethical issues associated with these weapons critical and relevant. ... Most research across disciplines unanimously agrees that it is immoral to detonate an atomic weapon due to both short and long-term catastrophic effects.

In fact, some scholars have concluded that it is therefore morally wrong to act in ways that produce these outcomes, which means it is morally wrong to engage in nuclear warfare.

Paladinen [302]3 years ago
5 0

Answer:

NO not at all.

Explanation:

After reading the accounts of people who survived the bomb in Hiroshima and Nagasaki in 1945 during World War II, I was horrified just <em>reading </em>the testimonies. <em>Almost</em> <em>every single</em> <em>survivor</em> described the skinless and bloated bodies they had seen everywhere. Inosuke Hayasaki, a surivor of the bombing, noticed one of his classmates, among many other citizens, pleading for water. When he tried listening for his heartbeat, his "skin slipped right off". Bombs are used in war so the other side will surrender<em>.</em> Bombs are aimed at "enemies" as if every being is an object to destroy. So no, bombing----let alone nuclear bombing----is ethical.

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Answer : The enthalpy of neutralization is, 56.012 kJ/mole

Explanation :

First we have to calculate the moles of HCl and NaOH.

\text{Moles of HCl}=\text{Concentration of HCl}\times \text{Volume of solution}=0.400mole/L\times 0.200L=0.08mol

\text{Moles of NaOH}=\text{Concentration of NaOH}\times \text{Volume of solution}=0.400mole/L\times 0.200L=0.08mol

The balanced chemical reaction will be,

HCl+NaOH\rightarrow NaCl+H_2O

From the balanced reaction we conclude that,

As, 1 mole of HCl neutralizes by 1 mole of NaOH

So, 0.08 mole of HCl neutralizes by 0.08 mole of NaOH

Thus, the number of neutralized moles = 0.08 mole

Now we have to calculate the mass of water.

As we know that the density of water is 1 g/ml. So, the mass of water will be:

The volume of water = 200mL+200L=400mL

\text{Mass of water}=\text{Density of water}\times \text{Volume of water}=1g/ml\times 400mL=400g

Now we have to calculate the heat absorbed during the reaction.

q=m\times c\times (T_{final}-T_{initial})

where,

q = heat absorbed = ?

c = specific heat of water = 4.18J/g^oC

m = mass of water = 400 g

T_{final} = final temperature of water = 27.78^oC=273+25.10=300.78K

T_{initial} = initial temperature of metal = 25.10^oC=273+27.78=298.1K

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

q=400g\times 4.18J/g^oC\times (300.78-298.1)K

q=4480.96J

Thus, the heat released during the neutralization = -4480.96 J

Now we have to calculate the enthalpy of neutralization.

\Delta H=\frac{q}{n}

where,

\Delta H = enthalpy of neutralization = ?

q = heat released = -4480.96 J

n = number of moles used in neutralization = 0.08 mole

\Delta H=\frac{-4480.96J}{0.08mole}=-56012J/mole=-56.012kJ/mol

The negative sign indicate the heat released during the reaction.

Therefore, the enthalpy of neutralization is, 56.012 kJ/mole

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