Use 'beta particle' in a sentence please.

What volume, in mL, of carbon dioxide gas is produced at STP by the decomposition of 0.242 g calcium carbonate (the products are

damaskus [11]

Answer:

54.21 mL.

Explanation:

We'll begin by calculating the number of mole in 0.242 g calcium carbonate, CaCO3.

This is illustrated below:

Mass of CaCO3 = 0.242 g

Molar mass of CaCO3 = 40 + 12 +(16x3) = 40+ 12 + 48 = 100 g/mol

Mole of CaCO3 =?

Mole = mass /Molar mass

Mole of CaCO3 = 0.242/100

Mole of CaCO3 = 2.42×10¯³ mole.

Next, we shall write the balanced equation for the reaction. This is given below:

CaCO3 —> CaO + CO2

From the balanced equation above,

1 mole of CaCO3 decomposed to produce 1 mole CaO and 1 mole of CO2.

Next, we shall determine the number of mole of CO2 produced from the reaction.

This can be obtained as follow:

From the balanced equation above,

1 mole of CaCO3 decomposed to produce 1 mole of CO2.

Therefore,

2.42×10¯³ mole of CaCO3 will also decompose to produce 2.42×10¯³ mole of CO2.

Therefore, 2.42×10¯³ mole of CO2 were obtained from the reaction.

Finally, we shall determine volume occupied by 2.42×10¯³ mole of CO2.

This can be obtained as follow:

1 mole of CO2 occupies 22400 mL at STP.

Therefore, 2.42×10¯³ mole of CO2 will occupy = 2.42×10¯³ x 22400 = 54.21 mL

Therefore, 54.21 mL of CO2 were obtained from the reaction.

7 0

3 years ago

. How many moles are there in 8.5x 1025 molecules of co2

bogdanovich [222]

1 mole => 6.023 x 10^23 molecules

x => 8.5 x 10^25 molecules

x = 8.5x10^25/ 6.023 x 10^23 = 141.1

6 0

3 years ago

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Please anyone answer this question

Ainat [17]

Answer:

A, 18.4 and 34!

Explanation:

The Burette seems to have ~18.4 of the liquid? substance in it, and the Measuring Cylinder seems to have ~34 of the liquid? substance in it. So, it is A! :]

Hope this helps!!

7 0

3 years ago

Suppose a 5.00 l sample of o2 at a given temperature and pressure contains 1.08

arsen [322]

Missing question: A 5.00 L sample of O2 at a given temperature and pressure contains a 1.08x10^23 molecules. How many molecules would be contained in each of the following at the same temperature and pressure? 
a) 5.00 L H2.
b) 5.00 L CO2.
Use Avogadro's Law: The Volume Amount Law: equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. Because hydrogen and carbon(IV) oxide are gases, number of molecules are the same as number of oxygen molecules, so:
a) N(H₂) = 1.08·10²³.
b) N(CO₂) = 1.08·10²³

5 0

3 years ago

Why would it be important for a scientist to understand HOW an element would react with another element?

Eddi Din [679]

Sounds good, but would do little to explain why lithium, with 3 electrons, is more reactive than Helium with 2, or why Caesium is more reactive than Sodium, although it clearly has far more electrons with which to shield its nucleus.

Hydrogen is unusual in having a fairly exposed nucleus, but chemistry is not very much about the nucleus, it is about the way the electrons themselves interact. As Lightarrow suggests, it does help if you know the quantum behaviour of electrons in an atom (which I do not claim to know), but it basically boils down to electrons preferring some configurations over others.

At the simplest, the comparison between hydrogen and helium – it is not really to do with the nucleus, it is more to do with electrons liking to be in pairs. Electrons have (like most common particles) two possible spin states, and they are more stable when an electron in one spin state is paired with an electron in the opposite spin state. When two hydrogen atoms meet, the electrons each one of them hold can be shared between them, forming a more stable pair of electrons, and thus binding the two atoms together.

All of the group 1 atoms (hydrogen, lithium, sodium, potassium, caesium; all share the characteristic that they have an odd number of electrons, and that one of those electrons is relatively unstable. The reason that the heavier atoms are more reactive is quite contrary to the argument that Lightarrow put forward – it is not because of a stronger electrical reaction with the nucleus, but because of the larger number of electrons in the bigger atoms, they are actually more weakly attached to their own nucleus, and so more readily interact with the electrons of other atoms.

Another, even more stable configuration for the electrons around an atom requires 8 electrons. This gives the noble gases (apart from Helium) their stability, but it also gives atoms like chlorine and fluorine their reactivity. Atoms like those of chlorine and fluorine are only one electron short of having a group 8 electrons available to them, and so will readily snatch an electron from another atom (particularly if it is an atom that has a single loose electron, such as sodium or caesium) in order to make up that group of 8 electrons.

The above explanation is very crude, and really does need a proper understanding of the quantum states of electrons to give a better quantitative answer (it is probably the kind of answer that might have been acceptable in the 1920s or 1930s – the Bohr orbital model of the atom, but has now been superseded by better explanations of what goes on amongst the electrons of an atom).

3 0

3 years ago

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