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3 years ago

29.) What charge would you expect from a Group 1 atom when it becomes an ion?

Chemistry

2 answers:

Veronika [31]3 years ago

8 0

Answer:

Explanation:

It is 1+ because when the periodic table is drawn well into there groups become cations

gavmur [86]3 years ago

8 0

The answer here would be d

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Which two compounds are molecules which both contain a double bond

Mademuasel [1]

Answer:

Double bond

Chemical compounds with double bonds.

Ethylene Carbon-carbon double bond.

Acetone Carbon-oxygen double bond.

Dimethyl sulfoxide Sulfur-oxygen double bond.

Diazene Nitrogen-nitrogen double bond.

Explanation:

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7 0

3 years ago

Why 1 mole of a gas (incompressible) contains 22400 ml of that substance?

saw5 [17]

Because that is the ideal gas at STP.

7 0

3 years ago

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds ________ M, BaF

BARSIC [14]

Answer:

When the concentration of F- exceeds 0.0109 M, BaF2 will precipitate.

Explanation:

Ba²⁺(aq) + 2 F⁻(aq) <----> BaF₂(s)

When BaF₂ precipitates, the Ksp relation is given by

Ksp = [Ba²⁺] [F⁻]²

[Ba²⁺] = 0.0144 M

[F⁻] = ?

Ksp = (1.7 × 10⁻⁶)

1.7 × 10⁻⁶ = (0.0144) [F⁻]²

[F⁻]² = (1.7 × 10⁻⁶)/0.0144 = 0.0001180555

[F⁻] = √0.0001180555 = 0.01086 M = 0.0109 M

Hope this Helps!!!

7 0

4 years ago

Each Excedrin tablet contains 250 mg aspirin (ACE), 250 mg of acetaminophen (ACE), and 65 mg of caffeine (CAF). Calculate the th

yawa3891 [41]

Answer:

a) 37.04% b) 37.04% c) 9.63%

Explanation:

The theoretical percent recovery (Tr), is the total percentage of each compound in the sample. Depending on the technique used to recovery the compounds, the percent recovery will be less than the theoretical, because no technique is 100% efficient.

So, to calculate the theoretical, it will be the mass of the compound divided by the mass of the sample multiplied by 100%.

a) Tr = (250 mg)/(675 mg) * 100%

Tr = 37.04%

b) Tr = (250 mg)/(675 mg) * 100%

Tr = 37.04%

c) Tr = (65 mg)/(675 mg) * 100%

Tr = 9.63%

3 0

4 years ago

How much energy is released by the decay of 3 grams of 230Th in the following reaction 230 Th - 226Ra + "He (230 Th = 229.9837 g

Serhud [2]

<u>Answer:</u> The energy released for the decay of 3 grams of 230-Thorium is $2.728\times 10^{-15}J$

<u>Explanation:</u>

First we have to calculate the mass defect $(\Delta m)$ .

The equation for the alpha decay of thorium nucleus follows:

$_{90}^{230}\textrm{Th}\rightarrow _{88}^{226}\textrm{Ra}+_2^{4}\textrm{He}$

To calculate the mass defect, we use the equation:

Mass defect = Sum of mass of product - Sum of mass of reactant

$\Delta m=(m_{Ra}+m_{He})-(m_{Th})$

$\Delta m=(225.9771+4.008)-(229.9837)=1.4\times 10^{-3}amu=2.324\times 10^{-30}kg$

(Conversion factor: $1amu=1.66\times 10^{-27}kg$ )

To calculate the energy released, we use Einstein equation, which is:

$E=\Delta mc^2$

$E=(2.324\times 10^{-30}kg)\times (3\times 10^8m/s)^2$

$E=2.0916\times 10^{-13}J$

The energy released for 230 grams of decay of thorium is $2.0916\times 10^{-13}J$

We need to calculate the energy released for the decay of 3 grams of thorium. By applying unitary method, we get:

As, 230 grams of Th release energy of = $2.0916\times 10^{-13}J$

Then, 3 grams of Th will release energy of = $\frac{2.0916\times 10^{-13}}{230}\times 3=2.728\times 10^{-15}J$

Hence, the energy released for the decay of 3 grams of 230-Thorium is $2.728\times 10^{-15}J$

5 0

3 years ago