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3 years ago

What is the mass of 5.35 mol of magnesium, Mg?

Chemistry

1 answer:

Hatshy [7]3 years ago

3 0

130.03175 g. Mol to mass is multiplication. So multiply 5.35 by 24.305 and you will get the answer

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Your dad is working on creating a brick border for the lake in your backyard each brick has a mass of 100 g and a volume of 20 c

wel

Answer:

5000kg/m³

Explanation:

density=mass/volume

d=m/v

d=100/20

=5g/cm³

g/cm³*1000=kg/m³

5g/m³*1000=5000kg/m³

4 0

3 years ago

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How many liters in 4.4 grams of CO2 at STP?

d1i1m1o1n [39]

Answer:

2.24 Liters are in 4.4 grams of CO2 at STP

5 0

3 years ago

In the reaction below, how many grams of h2o(g) are produced when 2.1 grams o2(g) are consumed? c4h6(g) + o2(g) → co2(g) + h2o(g

amm1812

The balanced equation that illustrates the reaction is:
2C4H6 + 11O2 ......> 8CO2 + 6H2O

number of moles = mass / molar mass
number of moles of oxygen = 2.1 / 32 = 0.065625 moles

Now, from the balanced equation, we can note that:
11 moles of oxygen are required to produce 6 moles of water.
Therefore:
0.065625 moles of oxygen will produce:
(0.065625*6) / 11 = 0.03579 moles of water

number of moles = mass / molar mass
mass = number of moles * molar mass
mass of water = 0.03579 * 18 = 0.644 grams

3 0

3 years ago

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Jkgergzruge˜©∫fghxtgrhxghzghgzhgzhmhrghgmhzh

DedPeter [7]

Sissy imposter among us haha

6 0

3 years ago

Tetrachloromethane, CCl4 is produced from the substitution reaction between methane and chlorine gas. If the rate of formation o

Korolek [52]

The rate of disappearance of chlorine gas : 0.2 mol/dm³

<h3>Further explanation</h3>

The reaction rate (v) shows the change in the concentration of the substance (changes in addition to concentrations for reaction products or changes in concentration reduction for reactants) per unit time.

For reaction :

$\tt aA+bB\rightarrow cC+dD$

The rate reaction :

$\tt -\dfrac{1}{a}\dfrac{d[-A]}{dt}= -\dfrac{1}{b}\dfrac{d[-B]}{dt}=\dfrac{1}{c}\dfrac{d[C]}{dt}=\dfrac{1}{d}\dfrac{d[D]}{dt}$

Reaction for formation CCl₄ :

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From equation, rate of reaction = rate of formation CCl₄ = 0.05 mol/dm³

Rate of formation of CCl₄ = reaction rate x coefficient of CCCl₄

0.05 mol/dm³ = reaction rate x 1⇒reaction rate = 0.05 mol/dm³

The rate of disappearance of chlorine gas (Cl₂) :

Rate of disappearance of Cl₂ = reaction rate x coefficient of Cl₂

Rate of disappearance of Cl₂ = 0.05 x 4 = 0.2 mol/dm³

4 0

3 years ago