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butalik [34]
3 years ago
12

Part a the sun produces energy via fusion. one of the fusion reactions that occurs in the sun is 411h→42he+201e how much energy

in joules is released by the fusion of 2.58 g of hydrogen-1? express your answer to three significant figures and include the appropriate units. view available hint(s) δe = submit part b this question will be shown after you complete previous question(s). return to assignment provide feedback
Chemistry
2 answers:
Orlov [11]3 years ago
4 0
The equation for the nuclear fusion reaction is,
4 ¹₁H → ₂⁴He + 2 ₁⁰e
Calculation of mass defect,
Δm = [mass of products - mass of reactants]
      = 4(1.00782) - [4.00260 + 2(0.00054858)]
      = 0.0275828 g/mole
Given that,
Mass of Hydrogen-1 = 2.58 g
The no. of moles of ₁¹H = 2.58 g / 1.00782 = 2.56 moles
Therefore, the mass defect for 2.58 g of ₁¹H is, 
= 2.56 moles * (0.0275828 g / 4) = 0.01765 x 10⁻³ kg
Energy for (0.01765 x 10⁻³ kg) is, 
= (0.01765 x 10⁻³ kg) (3.0 x 10⁸)² = 1.59 x 10¹² J
Anna007 [38]3 years ago
4 0

Answer:

Energy=-1.59x10^{12}J

Explanation:

Hello,

In this case, the requested energy is computed via the following equation, whereas the mass defected is the main issue to be calculated:

Energy=m_{d}*c^2

Whereas m_{d} is the mass defected and c the speed of light. In this manner, such mass is computed via:

m_d=m_{products}-m_{reagents}\\m_d=(mass_{He}+m_{electron})-4m_H

Now, given the mass of the H-1, He, and the electron, one computes such mass as shown below per 4 moles of H as those the involved moles:

m_d=4.00260g/mol+2*0.00054858g/mol-4*1.00782g/mol\\m_d=-0.027583g/4mol

Finally, we apply the firstly given formula for the determination of the energy, taking into account that to get Joules we need to convert the mass defected from grams to kilograms as follows:

Energy=2.58gH*\frac{1molH}{1.00782gH} *-0.027583gH/4molH*\frac{1kgH}{1000gH}*(299 792 458 m / s )^2\\Energy=-1.59x10^{12}J

The obtained energy turns out negative since is a released type of energy.

Best regards.

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5 0
3 years ago
If it takes 20.4 mL of NaOH(aq) to reach the equivalence point of the titration, what is the molarity of H2SO4(aq)? For your ans
Alik [6]

Question is incomplete, complete question is;

A 34.8 mL solution of H_2SO_4 (aq) of an unknown concentration was titrated with 0.15 M of NaOH(aq).

H_2SO_4(aq)+2NaOH(aq)\rightarrow Na_2SO_4(aq)+2H_2O(l)

If it takes 20.4 mL of NaOH(aq) to reach the equivalence point of the titration, what is the molarity of H_2SO_4(aq)? For your answer, only type in the numerical value with two significant figures. Do NOT include the unit.

Answer:

0.044 M is the molarity of H_2SO_4(aq).

Explanation:

The reaction taking place here is in between acid and base which means that it is a neutralization reaction .

To calculate the concentration of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is H_2SO_4

n_1,M_2\text{ and }V_2  are the n-factor, molarity and volume of base which is NaOH.

We are given:

n_1=2\\M_1=?\\V_1=34.8 mL\\n_2=1\\M_2=0.15 M\\V_2=20.4 mL

Putting values in above equation, we get:

2\times M_1\times 34.8 mL=1\times 0.15 M\times 20.4 mL\\\\M_1=\frac{1\times 0.15 M\times 20.4 mL\times 10}{2\times 34.8 mL}=0.044 M

0.044 M is the molarity of H_2SO_4(aq).

4 0
3 years ago
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