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Yanka [14]
4 years ago
6

Write the beta decay equation for the following isotope: 15/6 C?

Chemistry
1 answer:
vesna_86 [32]4 years ago
8 0

Answer:

\rm _{6}^{15}\text{C} \longrightarrow \,  _{-1}^{0}\text{e} + \,  _{7}^{15}\text{N}

Explanation:

The unbalanced nuclear equation is

\rm _{6}^{15}\text{C} \longrightarrow \,  _{-1}^{0}\text{e} + \, ?

Let's write the question mark as a nuclear symbol.

\rm _{6}^{15}\text{C} \longrightarrow \,  _{-1}^{0}\text{e} + \,  _{Z}^{A}\text{X}

The main point to remember in balancing nuclear equations is that the sums of the superscripts and the subscripts must be the same on each side of the equation.  

Then

15 =  0 + A, so A = 15 -   0 = 15, and

 6 = -1 + Z, so Z  =   6 + 1 =    7

Then, your nuclear equation becomes

\rm _{6}^{15}\text{C} \longrightarrow \,  _{-1}^{0}\text{e} + \,  _{7}^{15}\text{X}

Element 7 is nitrogen, so the balanced nuclear equation is

\rm _{6}^{15}\text{C} \longrightarrow \,  _{-1}^{0}\text{e} + \,  _{7}^{15}\text{N}

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The following reaction is exothermic.
earnstyle [38]

Answer : The correct option is, (C) spontaneous only at low temperatures.

Explanation :

According to Gibb's equation:

\Delta G=\Delta H-T\Delta S

\Delta G = Gibbs free energy  

\Delta H = enthalpy change

\Delta S = entropy change  

T = temperature in Kelvin

As we know that:

\Delta G= +ve, reaction is non spontaneous

\Delta G= -ve, reaction is spontaneous

\Delta G= 0, reaction is in equilibrium

The given chemical reaction is:

2S(s)+3O_2(g)\rightarrow 2SO_3(g)

As we are given that, the given reaction is exothermic that means the enthalpy change is negative.

In this reaction, the randomness of reactant molecules are more and as we move towards the formation of product the randomness become less that means the degree of disorderedness decreases. So, the entropy will also decreases that means the change in entropy is negative.

Now we have to determine the spontaneity of this reaction when ΔH is negative and ΔS is negative.

As, \Delta G=\Delta H-T\Delta S

\Delta G=(-ve)-T(-ve)

\Delta G=(+ve)   (at high temperature) (non-spontaneous)

\Delta G=(-ve)   (at low temperature) (spontaneous)

Thus, the reaction is spontaneous only at low temperatures.

4 0
3 years ago
You have a 0.7 M solution. Your job is to produce 50 mL of a 0.4 M solution.
Andreyy89

Answer: A. 28.6 ml of the 0.7 M solution we need to start with.

B. There are 0.02 moles of solute were in the 0.7 M solution.

C. Amount of water to be added is 21.4 ml

D. The resulting solution will have concentration of 0.28 M

Explanation:

According to the dilution law,

M_1V_1=M_2V_2

where,

M_1 = molarity of stock solution = 0.7 M

V_1 = volume of stock solution = ?

M_1 = molarity of diluted solution = 0.4 M

V_1 = volume of  diluted solution = 50 ml

Putting in the values we get:

0.7\times V_1=0.4\times 50

V_1=28.6ml

A. 28.6 ml of the 0.7 M solution we need to start with.

B. Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

Molarity=\frac{n\times 1000}{V_s}

where,

n = moles of solute

V_s = volume of solution in ml

0.7=\frac{n\times 1000}{28.6}

n=0.02

Thus there are 0.02 moles of solute were in the 0.7 M solution.

C. Amount of water to be added = (50-28.6 ) ml = 21.4 ml

D. If water added is 2\times 21.4=42.8 ml

0.7\times 28.6=M_2\times 71.4

M_2=0.28M

If volume of concentrated solution will be more , the resulting solution will have lesser concentration of 0.28 M

8 0
3 years ago
What is displacement?
mars1129 [50]
Displacement reaction is a chemical reaction in which a more reactive element displaces a less reactive element from its compound. Both metals and non-metals take part in displacement reactions. Example : Reaction of iron nails with copper sulphate solution.
8 0
3 years ago
Respiration describes the process that living cells use to release energy by combining sugar and oxygen. The primary chemical ch
True [87]

Answer:

C the mass of the reactant molecules is the same as the mass of the product

5 0
3 years ago
Next the students measured the density of aluminum metal. The accepted density for aluminum is 2.7 g/cm3. The students collected
katovenus [111]

Answer:

yo that's too long you should try and my it shorter

3 0
4 years ago
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