The chemical changes that occur as a car ages are fading of paint due to sunlight. rusting on the chrome, corrosion of electrical wiring. Some physical changes that occur as a car ages are breaking of the handles and straps, wearing down of tyre, paint scratches.
A chemical change is one which brings change in the composition of the substance. In other words, it is such a change which forms a completely new substance or product. It is an irreversible change.
On the other hand, a physical change is one which brings structural change or change in appearance of a substance without changing its original composition. It is a reversible change.
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Answer:physical: a part falling off or changing a tire. chemical:rust
Explanation:
B: our solar system
C: chocolate chip cookie
dough
D: the Milky Way galaxy
A. Plum Pudding
This is also a simple google search
This is a unit conversion problem. Nm (nanometer) is smaller than mm (millimeter).
1 mm = 1/10³m = 1 x 10⁻³ m
1 nm = 1/10⁹ m = 1 x10⁻⁹ m
1 m = 1 x 10⁹ nm
Hence, 2 mm = 2 x 10⁻³ m
Then we can convert 2 x 10⁻³ m to nm by multiplying with 10⁹.
Then 2 mm = 2 x 10⁻³ m = 2 x 10⁻³ x 10⁹ nm = 2 x 10⁶ nm.
Hence, the thickness of nickel is 2 x 10⁶ nm.
Answer: STP
CaCO3 = 5 g
Convert gram to mol
100 g of CaCO3 = 1 mol
5 g of CaCO3 (n) = 5 g *(1 mol/100 g) = 0.05 mol
Gas law
PV =nRT
V = nRT/P
V = (0.05 mol * (0.08206 L atm /K mol) *273 K)/1 atm
V = 1.124 L
Explanation:
When 5.0 g of CaCO3 are treated with excess hydrochloric acid, it forms 1.118 L of CO2 gas at STP.
When 5.0 g of CaCO3 is treated with excess hydrochloric acid, it undergoes a chemical reaction and forms CO2 gas. To find the number of liters of CO2 formed at STP (standard temperature and pressure), we need to use the ideal gas law. The molar mass of CaCO3 is 100.09 g/mol, and 1 mol of CaCO3 produces 1 mol of CO2 gas. The volume of 1 mol of any gas at STP is 22.4 L. Therefore, we can calculate the number of moles of CaCO3, then convert it to moles of CO2 and finally to the volume of CO2 gas in liters.
Using the given information, we have:
Mass of CaCO3 = 5.0 g
Molar mass of CaCO3 = 100.09 g/mol
Moles of CaCO3 = Mass of CaCO3 / Molar mass of CaCO3
Moles of CO2 = Moles of CaCO3
Volume of CO2 at STP = Moles of CO2 * 22.4 L/mol
Plugging in the values, we get:
Moles of CaCO3 = 5.0 g / 100.09 g/mol = 0.04997 mol
Moles of CO2 = 0.04997 mol
Volume of CO2 at STP = 0.04997 mol * 22.4 L/mol = 1.118 L
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sample containing a mixture of only these
gases at exactly one atmosphere pressure, the
partial pressures of carbon dioxide and ni-
trogen are given as Pco, = 0.285 torr and
PN = 634.034 torr. What is the partial pres-
sure of oxygen?
Answer in units of torr.
Answer:
125.681 torr
Explanation:
The formula to calculate the partial pressure of oxygen:
P(O2) = Pcommon - PCO2 - PN2
1 atm = 760 torr
Therefore you need to find the partial pressure of oxygen:
P(O2) = 760 torr -0.285 torr - 634.034 torr =130.013 torr
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The answer is: the atom with more valence electrons are in the middle of a molecule and it form more bonds.
For example, molecule hydrogen cyanide (HCN).
Lewis structure for hydrogen cyanide is H:C:::N:
Hydrogen has valence one (I), it means it has one single bond and electron configuration like closest noble gas helium.
Carbon has valence four (IV), it has four bonds (one with hydrogen and three with nitrogen) and full octet.
Nitron has valence three (III), it has full octet and electron configuration like noble gas neon (Ne).
Hydrogen cyanide has linear shape (the bond angles of 180 degrees).