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3 years ago

Solve the science problem No spamming

Chemistry

1 answer:

N76 [4]3 years ago

8 0

Answer:

the fastest would be gas, liquid would be in the middle and solid would be the slowest

Explanation:

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C= 51.89% H= 9.82% Br=38.29%

maks197457 [2]

Answer:

Explanation:

3 0

3 years ago

What volume of oxygen gas is released at STP if 10.0 g of potassium chlorate is decomposed? (The molar mass of KClO3 is 122.55 g

ArbitrLikvidat [17]

KClO3(s)+Δ→KCl(s)+32O2(g)

Approx. 3L of dioxygen gas will be evolved.

Explanation:

We assume that the reaction as written proceeds quantitatively.

Moles of KClO3(s) = 10.0⋅g122.55⋅g⋅mol−1 = 0.0816⋅mol

And thus 32×0.0816⋅mol dioxygen are produced, i.e. 0.122⋅mol.

At STP, an Ideal Gas occupies a volume of 22.4⋅L⋅mol−1.

And thus, volume of gas produced = 22.4⋅L⋅mol−1×0.0816⋅mol≅3L

Note that this reaction would not work well without catalysis, typically MnO2.

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3 years ago

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Harriet has an itch in her throat, and she begins to cough. she reaches for a cup of water to drink. which action is carried out

Nikitich [7]

when she reaches for the cup that is somatic nervous system. when she begins to cough

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3 years ago

An automobile can travel 40.0 miles on one gallon of gasoline how many kilometers per liter is this

Dmitrij [34]

Sent a pic of your problem and worked it out.

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3 years ago

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A 0.216 g sample of carbon dioxide, CO2, has a volume of 507 mL and a pressure of 470 mmHg. What is the temperature of the gas i

Gala2k [10]

Answer:

The temperature of the gas is 876.69 Kelvin

Explanation:

Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P*V = n*R*T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.

In this case:

P= 470 mmHg
V= 570 mL= 0.570 L
n= 0.216 g= 0.0049 moles (being the molar mass of carbon dioxide is 44 g/mole)

R= 62.36367 $\frac{mmHg*L}{mol*K}$

Replacing:

470 mmHg*0.570 L= 0.0049 moles* 62.36367 $\frac{mmHg*L}{mol*K}$ *T

Solving:

$T=\frac{470 mmHg*0.570 L}{0.0049 moles* 62.36367\frac{mmHg*L}{mol*K} }$

T= 876.69 K

The temperature of the gas is 876.69 Kelvin

6 0

3 years ago