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krek1111 [17]
3 years ago
7

What type of radiation is emitted when chromium-51 decays into manganese-51? Show the nuclear equation that leads you to this an

swer
Chemistry
2 answers:
tester [92]3 years ago
5 0

Answer is : beta (minus) decay.

Beta decay is radioactive decay in which a beta ray and a neutrino are emitted from an atomic nucleus.  

There are two types of beta decay: beta minus and beta plus.  

In beta minus decay (this example), neutron is converted to a proton, an electron and an electron antineutrino and decay atomic number Z is increased by one.

Nuclear equation: 51/24Cr → 61/25Mn+ 0/+1e.

Anastasy [175]3 years ago
4 0
It's a beta decay
24Cr51 --> 25Mn51 + -1eo
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In this section, you learned about pressure in fluids. Answer the question that follows.
Serga [27]

I think that the answer might be B.

7 0
3 years ago
What is the Name of RbC2H3O2
Semenov [28]

Answer:

Rubidium Acetate

Explanation:

Rb is Rubidium C2H3O2 is acetate

4 0
3 years ago
Read 2 more answers
Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant o
sattari [20]

Answer:

4.26 %

Explanation:

There is some info missing. I think this is the original question.

<em>Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is  4.50  ×  10 ⁻⁴.</em>

<em />

Step 1: Given data

Initial concentration of the acid (Ca): 0.249 M

Acid dissociation constant (Ka): 4.50  ×  10 ⁻⁴

Step 2: Write the ionization reaction for nitrous acid

HNO₂(aq) ⇒ H⁺(aq) + NO₂⁻(aq)

Step 3: Calculate the concentration of nitrite in the equilibrium ([A⁻])

We will use the following expression.

[A^{-} ] = \sqrt{Ca \times Ka } = \sqrt{0.249 \times 4.50 \times 10^{-4}  } = 0.0106 M

Step 4: Calculate the percent ionization of nitrous acid

We will use the following expression.

\alpha = \frac{[A^{-} ]}{[HA]} \times 100\% = \frac{0.0106M}{0.249} \times 100\% = 4.26\%

4 0
3 years ago
You add 7.8 g of iron to 20.70 mL of water and observe that the volume of iron and water together is 21.69 mL . Calculate the de
bixtya [17]
21.69mL - 20.70mL = .99mL Fe
7.8 g / .99 mL = 7.9g/mL 
4 0
3 years ago
White vinegar is a 5.0% by mass solution of acetic acid in water. If the density of white
Alex_Xolod [135]

The pH = 2.41

<h3>Further explanation</h3>

Given

5.0% by mass solution of acetic acid

the density of white  vinegar is 1.007 g/cm3

Required

pH

Solution

Molarity of solution :

\tt M=\dfrac{\%mass\times \rho\times 10}{MW~acetic~acid}\\\\M=\dfrac{5\times 1.007\times 10}{60}\\\\M=0.839

Ka for acetic acid = 1.8 x 10⁻⁵

[H⁺] for weak acid :

\tt [H^+]=\sqrt{Ka.M}

Input the value :

\tt [H^+]=\sqrt{1.8\times 10^{-5}\times 0.839}\\\\(H^+]=0.00388=3.88\times 10^{-3}\\\\pH=3-log~3.88=2.41

7 0
3 years ago
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