The modern atomic model states that electrons move sort of like what?

Which is the fastest in the universe apart from the light

Salsk061 [2.6K]

Well i did some research and i found out now im not sure if this is completely true but supposedly tachyons are even faster than the speed of light

3 0

3 years ago

LICUICY NICULUM

Evgen [1.6K]

Answer:

Missing component

Cl₂

H₂O

Explanation:

Reaction given:

? + 2NaBr → 2NaCl+Br

Mg+? → MgO+H2

missing component = ?

Solution:

Reaction 1

? + 2NaBr -----→ 2NaCl + Br

if we look at the reactants and products there is one element is in product side but not shown in the reactant side.

In products there are following atoms

Na (Sodium)

Cl (Chlorine)

Br (Bromine)

In Reactant there are following atoms

Na (Sodium)

Br (Bromine)

So only Chlorine is missing in the reactant side.

if we put chlorine in the reactant then this reaction will be complete

Cl + 2 NaBr -----→ 2NaCl + Br

So chlorine react with water and give sodium chloride and bromine molecule, this is a single displacement reaction and chlorine replace bromine in the above reaction

Now balance the equation

Cl₂ + 2 NaBr -----→ 2NaCl + Br₂

So, the missing component is

Cl₂

____________

Reaction 2

Mg + ? ---------→ MgO + H₂

if we look at the reactants and products there are two element in product side but not shown in the reactant side.

In products there are following atoms

Mg (Magnesium)

O (Oxygen)

H (Hydrogen)

In Reactant there is only one following atom

Mg (Magnesium)

So Oxygen and Hydrogen is missing in the reactant side.

if we put water molecule (H₂O) in the reactant then this reaction will be complete

Mg + H₂O ---------→ MgO + H₂

in this reaction magnesium (Mg) react with water (H₂O) and give magnesium oxide and hydrogen gas.

So, the missing component is

H₂O

3 0

3 years ago

Read 2 more answers

Calculate the number of O atoms in 0.364 g of CaSO4 · 2H2O

Nikolay [14]

Answer:

= 7.66 x 10²¹ oxygen atoms in 0.364 grams of CaSO₄·2H₂O

Explanation:

For problems like this posting, one needs an understanding of the following topics:

The definition of the mole

1 mole of substance = mass in grams of substance containing 1 Avogadro's Number ( = 6.023 x 10²³ ) of particles of the specified substance. This is generally one formula weight of the substance of interest. From this, the following equivalent relationships should be memorized:

1 mole = 1 formula weight = 1 mole weight (g)= 6.023 x 10²³ particles

Converting grams to moles:

Given grams => moles = grams/gram formula wt

Converting moles to grams:

Given moles => grams = moles x gram formula wt

_________________________________________________________

Calculate the number of O atoms in 0.364 g of CaSO₄ · 2H₂O.

Given mass CaSO₄ · 2H₂O = 0.364 grams

Formula Wt CaSO₄ · 2H₂O = 172 g/mole

moles CaSO₄ · 2H₂O = mass CaSO4 · 2H2O / formula Wt. CaSO₄ · 2H₂O

= 0.364 g CaSO₄·2H₂O / 172 g CaSO4·2H2O

= (0.364/172) mole CaSO₄·2H₂O

= 2.12 x 10⁻³ mole CaSO₄·2H₂O

∴ number of Oxy (O) atoms in 0.364 grams CaSO₄·2H₂O

= (2.12 x 10⁻³ mole CaSO₄ · 2H₂O)(6.023 x 10²³ molecules CaSO₄· 2H₂O/ mole)

= 1.276876 x 10²¹molecules CaSO₄· 2H₂O CaSO₄2H₂O

= 1.276876 x 10²¹ molecules CaSO₄· 2H₂O x 6 oxygen atoms / molecule

= 7.661256 x 10²¹ oxygen atoms in 0.364 grams of CaSO₄·2H₂O

= 7.66 x 10²¹ oxygen atoms in 0.364 grams of CaSO₄·2H₂O

8 0

2 years ago

Mrs. Smith is demonstrating a chemical change for her class. She places 15 grams of baking soda into a beaker. Next she adds 15

vichka [17]

According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.

∴ B is the Answer

4 0

3 years ago

Read 2 more answers

In a chemistry laboratory, a student filled a 10.0 L container with two (2) different gases. The

alexgriva [62]

Answer:

$P_N=1.33atm\\\\P_O=0.67atm$

$P_T=2.00 atm$

Explanation:

Hello.

In this case, the first step is to compute the moles of nitrogen and oxygen given their initial P, T and V conditions via the ideal gas equation:

$n_{N}=\frac{P_{N}V_{N}}{RT} =\frac{2.00atm*24.0L}{0.082\frac{atm*L}{mol*K}*273K}\\ \\n_{N}=2.144molN\\\\n_{O}=\frac{P_{O}V_{O}}{RT} =\frac{2.00atm*12.0L}{0.082\frac{atm*L}{mol*K}*273K}\\ \\n_{O}=1.072molO$

After that, since the total volume now, once the mixture is formed is the addition between the initial volumes (12.0 L + 24.0 L) is 36.0 L, the partial pressure of each gas turns out:

$P_N=\frac{2.144mol*0.082\frac{atm*L}{mol*K}*273K}{36.0L}\\\\P_N=1.33atm\\\\P_O=\frac{1.072mol*0.082\frac{atm*L}{mol*K}*273K}{36.0L}\\\\P_O=0.67atm$

Thus, the final total pressure is:

$P_T= P_N+P_O=1.33atm+0.67atm\\\\P_T=2.00 atm$

Best regards.

3 0

3 years ago