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Julli [10]
3 years ago
10

1

Chemistry
1 answer:
antoniya [11.8K]3 years ago
6 0
Amount of space an object takes up
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What are reasons standardizing conditions in which chemist describe matter?
ExtremeBDS [4]
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7 0
3 years ago
How will the candle contributes to the pressure and temperature of gases inside the glass?
Tems11 [23]
How will the candle contributes to the pressure and temperature of gases inside the glass?

The candle contributes to the pressure and temperature of the gases inside the glass because of the increasing temperature the lit of the candle disposes into the gas molecules inside and as these gas molecules rise in temperature they become unsettling and since heat makes gas molecules robust the area becomes smaller for them to be ecstatic and as the dynamics is explained p=f/a the pressure increases.

7 0
3 years ago
HELP PLS PLS PLS ILL MARK U BRAINLIEST
777dan777 [17]

Answer:

2 FeCl3 → 2 Fe + 3 Cl2

Explanation:

2 Fe and 6 Cl on the reactants side, and 2 Fe and 6 Cl on the products side.

7 0
2 years ago
A gas mixture of Ne and Ar has a total pressure of 4.00 atm and contains 16.0 mol of gas. If the partial pressure of Ne is 2.75
Stolb23 [73]

Answer:

5 moles of Argon is present in the mixture.

Explanation:

Total pressure of the gaseous mixture = 4 atm

Total number of moles = 16

Partial pressure of Ne = 2.75 atm

By Dalton's law of partial pressure, the total pressure of gaseous mixture is the sum of partial pressures of individual gases which are non-reactive.

Hence:

P_{total}=P_{Ar}+P_{Ne}\\4=P_{Ar}+2.75\\P_{Ar}=1.25\ atm

Also :

Partial pressure = mole fraction*total pressure

P_{Ar}=X_{Ar}P_{total}

X_{Ar}=\frac{1.25}{4}=0.3125

\frac{n_{Ar}}{n_{total}}=0.3125\\n_{Ar}=5

∴Number of moles of Argon = 5

4 0
3 years ago
I’ll mark as brainliest
zysi [14]

First, let's count mole of 10 g Calcium Carbonate

mole = Mass / Molecular Mass

Calcium Carbonate = CaCO₃

Molecular Mass = Ar Ca + Ar C + (3 x Ar O)

Molecular Mass = 40 + 12 + (3 x 16)

Molecular Mass = 100

next

Mole of CaCO₃ = 10 gram / 100

Mole of CaCO₃ = 0,1 mol

then equal the reaction equation first

 CaCO₃ + 2 HCl  ==>  CaCl₂ +  CO₂  +  H₂O     (Equal)

To count the mass of carbon dioxide that produced we must know the mole of CO₂ first

we can count by coefficient comparison

mole CO₂ = \frac{coefficient \ of \ CO_2}{coefficient \ of \ CaCO_3}  x mole CaCO₃

mole  CO₂ =  (1/1)  x 0,1 mole

mole  CO₂ = 0,1 mole

so

Mass of  CO₂ = mole  CO₂ x  Molecular Mass of  CO₂

Mass of  CO₂ = 0,1 mole x (12 + (2 x 16))

Mass of  CO₂ = 0,1 mole x 44

Mass of  CO₂ = 4,4 g

so, mass of carbon dioxide that's produced by 10 g of calcium carbonate on reaction with chloride acid is 4,4 g.

6 0
3 years ago
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