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MatroZZZ [7]
3 years ago
6

Question 54

Chemistry
1 answer:
dusya [7]3 years ago
7 0
I really hope and think it’s E
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What is the term<br>chemistry​
kotegsom [21]

Answer:

Chemistry is the scientific study of the structure of substances, how they react when combined and how they behave under different situations.

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3 years ago
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Density,mass,volume: Is the amount of matter a substance has
LuckyWell [14K]
Density is the mass of a substance per unit volume. Volume is the amount of space an object occupies. Chemical properties- These are properties that can only be observed by changing the identity of the substance

Hope it helped ya out!
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Given the number of a substance , how do you solve for the number of a moles of a substance
chubhunter [2.5K]
Given the number of a substance, we can solve the number of moles by using a conversion factor that would relate the number of a substance to the number of moles. In any case, Avogadro's number would be used. It <span>represents the number of units in one mole of any substance. This has the value of 6.022 x 10^23 units / mole. This number can be used to convert the number of atoms or molecules into number of moles. For example, we are given 1.23 x 10^24 atoms of a substance converting it to moles we do as follows:

 </span>1.23 x 10^24 atoms ( 1 mol / 6.022x10^23 atoms ) = 2.04 moles
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3 years ago
There are 342 g of sucrose in 1.00 mol of sucrose. What is the molar concentration (molarity) of a solution containing 171 g suc
Elodia [21]
To get the molarity, you divide the mass in moles over the amount in liters. To convert the grams to moles, divide the amount of grams by the molar mass. In this case, I believe sucrose has a molar mass of 342.297. Once you divide 171/342.297 you should get .4996. Now divide that by the .750 to get a final answer of .6660. Check to make sure you don't have to follow the significant figure rules.
7 0
3 years ago
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CaCO3(s)⇄CaO(s)+CO2(g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxid
rusak2 [61]

Answer:

1.04 mol

Explanation:

CO₂ is produced in a closed 100 L vessel according to the following equation.

CaCO₃(s) ⇄ CaO(s) + CO₂(g)

At equilibrium, the pressure of carbon dioxide remains constant at 1.00 atm.

First, we need to conver the temperature to the absolute scale (Kelvin scale) using the following expression.

K = °C + 273.15

K = 898°C + 273.15

K = 1171 K

Now, we can find the moles of carbon dioxide using the ideal gas equation.

P \times V = n \times R \times T\\n = \frac{P \times V}{R \times T} = \frac{1.00atm \times 100L}{\frac{0.0821atm.L}{mol.K}  \times 1171K} = 1.04 mol

7 0
3 years ago
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