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sweet-ann [11.9K]
3 years ago
9

The radioactive atom 61/27 co emits a beta particle. write an equation showing the decay

Chemistry
1 answer:
pickupchik [31]3 years ago
7 0

Answer:

\rm _{27}^{60}\text{Co} \longrightarrow \,  _{-1}^{0}\text{e} + \, _{28}^{60}\text{Ni}

Explanation:

The unbalanced nuclear equation is

\rm _{27}^{60}\text{Co} \longrightarrow \,  _{-1}^{0}\text{e} + \, ?

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

\rm _{27}^{60}\text{Co} \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

60 = 0 + A, so A = 60 - 0 = 60, and

27 = -1 + Z, so Z  = 27 + 1 = 28

Your nuclear equation becomes

\rm _{27}^{60}\text{Co} \longrightarrow \,  _{-1}^{0}\text{e} + \, _{28}^{60}\text{X}

Element 28 is nickel, so the balanced nuclear equation is

\rm _{27}^{60}\text{Co} \longrightarrow \,  _{-1}^{0}\text{e} + \, _{28}^{60}\text{Ni}

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3 0
3 years ago
Que. 1. Gallium has 2 naturally occuring Isotopes with mass numbers 69 &amp; 71 respectively. What is the percentage abundance o
IgorC [24]

Isotopes are atoms of the same element that have different masses. The relative atomic mass (am) is a weighted average that takes into account the abundance of each isotope. We can calculate the relative atomic mass using the following expression.

am = \frac{\Sigma m_i  \times ab_i}{100}

where,

  • mi: mass of each isotope
  • abi: percent abundance of each isotope

For Gallium,

70.59 amu = \frac{69 amu\ x + 71 amu\ y}{100}     [1]

where "x" and "y" are the unknown abundances.

We also know that the sum of both abundances must be 100%.

x + y = 100

y = 100 - x   [2]

If we replace [2] in [1], we get

70.59 amu = \frac{69 amu\ x + 71 amu\ (100-x)}{100} \\7059 amu = -2 amu\ x + 7100amu \\x = 20.5

Then, in [2]

y = 100 - x = 100 - 20.5 = 79.5

In conclusion, Ga-69 has an abundance of 20.5% and Ga-71 has an abundance of 79.5%.

You can learn more about isotopes in: brainly.com/question/21536220?referrer=searchResults

7 0
3 years ago
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7 0
3 years ago
Consider the reaction. mc015-1.jpg How many grams of N2 are required to produce 100.0 L of NH3 at STP?
Nadusha1986 [10]
The  grams  of N2  that  are   required   to  produce 100.0 l  of  NH3   at  STP

At  stp 1moles = 22.4  l. what  about  100.0 L of NH3

= 100 / 22.4 lx1  moles = 4.46  moles  of NH3

write the reacting  equation

N2+3H2 =2NH3
by use of mole  ratio  between  N2  to NH3  which is  1:2 the moles of N2 =4.46/2 =2.23  moles of N2

mass =  moles  x  molar  mass

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3 0
3 years ago
The following chemical reaction occurs in a basic solution.
Dafna1 [17]

Answer:

6 moles of electrons

Explanation:

Let us consider the species NO3− and ClO−. The NO3− is oxidized to NO the oxidation number of nitrogen is decreased from +5 to +2.

The oxidation number of chlorine is increased from +1 to +3. This implies that six electrons were transferred in the balanced reaction equation shown in the question. Hence the answer.

3 0
3 years ago
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