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-Dominant- [34]
3 years ago
13

Look at the diagram of the atom. What will it change to during beta decay? A)An atom with 3 protons, 4 neutrons, and 3 electrons

B)An atom with 3 protons, 4 neutrons, and 4 electrons C)An atom with 4 protons, 3 neutrons, and 4 electrons D)An atom with 4 protons, 3 neutrons, and 3 electrons

Chemistry
1 answer:
GREYUIT [131]3 years ago
5 0
D) An atom with 4 protons, 3 neutrons, and 3 electrons
You might be interested in
A buffer consists of 0.120 M HNO2 and 0.150 M NaNO2 at 25°C. pka of HNO2 is 3.40. a. What is the pH of the buffer? b. What is th
Mashcka [7]

Explanation:

It is known that K_{a} of HNO_{2} = 4.5 \times 10^{-4}.

(a)  Relation between K_{a} and pK_{a} is as follows.

                       pK_{a} = -log (K_{a})

Putting the values into the above formula as follows.

                      pK_{a} = -log (K_{a})

                                    = -log(4.5 \times 10^{-4})

                                     = 3.347

Also, relation between pH and  pK_{a} is as follows.

              pH = pK_{a} + log\frac{[conjugate base]}{[acid]}

                     = 3.347+ log \frac{0.15}{0.12}

                    = 3.44

Therefore, pH of the buffer is 3.44.

(b)   No. of moles of HCl added = Molarity \times volume

                                            = 11.6 M \times 0.001 L

                                             = 0.0116 mol

In the given reaction, NO^{-}_{2} will react with H^{+} to form HNO_{2}

Hence, before the reaction:

No. of moles of NO^{-}_{2} = 0.15 M \times 1.0 L

                                           = 0.15 mol

And, no. of moles of HNO_{2} = 0.12 M \times 1.0 L

                                               = 0.12 mol

On the other hand, after the reaction :  

No. of moles of NO^{-}_{2} = moles present initially - moles added

                                          = (0.15 - 0.0116) mol

                                          = 0.1384 mol

Moles of HNO_{2} = moles present initially + moles added

                               = (0.12 + 0.0116) mol

                                = 0.1316 mol

As, K_{a} = 4.5 \times 10^{-4}

           pK_{a} = -log (K_{a})

                         = -log(4.5 \times 10^{-4})

                         = 3.347

Since, volume is both in numerator and denominator, we can use mol instead of concentration.

As, pH = pK_{a} + log \frac{[conjugate base]}{[acid]}

            = 3.347+ log {0.1384/0.1316}

            = 3.369

            = 3.37 (approx)

Thus, we can conclude that pH after the addition of 1.00 mL of 11.6 M HCl to 1.00 L of the buffer solution is 3.37.

6 0
3 years ago
A sample of gas has a volume of 75.0 mL at 30.0 psi. Determine the pressure of the gas if its volume is changed to 15 mL and its
Assoli18 [71]

Answer:

5.995 psi

Explanation:

30 psi = 2.04 atm

75 mL = 0.075 L

15 mL = 0.015 L

0.075 L/ 2.04 atm = 0.015 L/x

0.075x = 0.0306

x = 0.408

0.408 atm = 5.995 psi

4 0
3 years ago
Sodium carbonate reacts with silver nitrate according to the following balanced equation: Na2CO3 (s) + 2 AgNO3 (aq) → Ag2CO3 (s)
klemol [59]

Answer:

a) 2.01 g

Explanation:

  • Na₂CO₃ (s) + 2AgNO₃ (aq) → Ag₂CO₃ (s) + 2NaNO₃

First we <u>convert 0.0302 mol AgNO₃ to Na₂CO₃ moles</u>, in order to <em>calculate how many Na₂CO₃ moles reacted</em>:

  • 0.0302 mol AgNO₃ * \frac{1molNa_2CO_3}{2molAgNO_3}  = 0.0151 mol Na₂CO₃

So the remaining Na₂CO₃ moles are:

  • 0.0340 - 0.0151 = 0.0189 moles Na₂CO₃

Finally we <u>convert Na₂CO₃ moles into grams</u>, using its <em>molar mass</em>:

  • 0.0189 moles Na₂CO₃ * 106 g/mol = 2.003 g Na₂CO₃

The closest answer is option a).

8 0
3 years ago
2. A 2.5 mol SAMPLE OF OXYGEN GAS (O2) INCREASES TO 3.2 mol
lana [24]

696.32 mmHg is the final pressure of the gas.

<h3>What is an ideal gas equation?</h3>

The ideal gas equation, pV = nRT, is an equation used to calculate either the pressure, volume, temperature or number of moles of a gas.

Given data:

P_1 = 720 mmHg              

P_2 = ?

n_1 = 2.5 mol                

n_2 = 3.2 mol

V_1 = 34 L            

V_2 = 45 L

Formula

Combined gas law

\frac{P_1 V_1}{n_1}  = \frac{P_2 V_2}{n_2}

P_2 = 696.32 mmHg

Hence, 696.32 mmHg is the final pressure of the gas.

Learn more about an ideal gas equation here:

brainly.com/question/19251972

#SPJ1

6 0
2 years ago
When a hurricane approaches land, people living directly on the
Tatiana [17]

Answer:

True

Explanation:

When a hurricane is dangerous enough that authorities say to evacuate, you should for your own safety.

3 0
3 years ago
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