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2 years ago

Antoine Henri Becquerel discovered radioactivity when he was studying

Chemistry

2 answers:

Katen [24]2 years ago

5 0

Antoine Henri Becquerel discovered radioactivity when he was studying

X- rays.

He had been studying phosphorescent uranium ores and hypothesized that they might absorb sunlight and reemit it as X-rays.

His hypothesis was wrong, but his experiments led to the discovery of natural radioactivity.

Gemiola [76]2 years ago

3 0

X-Rays is the answer

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Chlorine forms a number of oxides with the following oxidation numbers: 1, 3, 4, 6, and 7. These compounds are stable and neutra

SashulF [63]

Answer:

$Cl_2O$ , $Cl_2O_3$ , $ClO_2$ , $ClO_3$ , $Cl_2O_7$

Explanation:

Empirical formula of the compound is the simplest ratio of elements present in the compound.

Empirical formula of compounds of chlorine with oxygen is as follows:

Compounds in which oxidation state of Cl is +1

$Cl_2O$

Compounds in which oxidation state of Cl is +3

$Cl_2O_3$

Compounds in which oxidation state of Cl is +4

$ClO_2$

Compounds in which oxidation state of Cl is +6

$ClO_3$

Compounds in which oxidation state of Cl is +7

$Cl_2O_7$

8 0

2 years ago

What happens to the individual molecules of a liquid as they gain enough kinetic energy to escape the surface of the liquid?

Bumek [7]

Im pretty sure They freeze

7 0

2 years ago

Read 2 more answers

Given the equation:

Archy [21]

X will be hydronium (H3O)

3 0

2 years ago

Read 2 more answers

What is the mass of bromine gas if it has a pressure of 720 mmHg, volume of 25mL and a temperature of 18.3 degrees Celsius

Annette [7]

Answer:

Mass = 0.158 g

Explanation:

Formula used,

P V = n R T

Or,

n = P V / R T

Putting values,

n = 0.948 atm . 0.025 L / 0.0821 L.atm.K⁻¹.mol⁻¹ . 291.45

n = 0.00099 mol

Note: we have changed pressure from mmHg to atm, volume from mL to L and temperature from C to K)

Also,

Mass = n . Molecular Mass

Mass = 0.00099 mol × 159.808 g/mol

Mass = 0.158 g

7 0

1 year ago

An unknown amount of mercury (II) oxide was decomposed in the lab. Mercury metal was formed and 5.20 L of oxygen was released at

Yakvenalex [24]

Answer:

68.3g

Explanation:

1. Word equation:

mercury(II) oxide → mercury + oxygen

2. Balanced molecular equation:

2HgO → 2Hg + O₂(g)

3. Mole ratio

Write the ratio of the coefficients of the substances that are object of the problem:

$2molHgO/1molO_2$

4. Calculate the number of moles of O₂(g)

Use the equation for ideal gases:

$pV=nRT\\\\\\n=\dfrac{pV}{RT}\\\\\\n=\dfrac{0.970atm\times5.20L}{0.08206atm.L/K.mol\times 390.0K}\\\\\\n=0.1576mol$

5. Calculate the number of moles of HgO

$\dfrac{2molHgO}{1molO_2}\times 0.1576molO_2=0.315molHgO$

6. Convert to mass

mass = # moles × molar mass

molar mass of HgO: 216.591g/mol

mass = 0.315mol × 216.591g/mol = 68.3g

7 0

2 years ago