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2 years ago

Identify the molecule that effuses the fastest ch4 co ar or co2

2 answers:

5 0

<span>CH4 will effuse the fastest. The speed of effusion is proportional to the speed of the gas molecules with faster molecules effusing fast than slower molecules. And the speed of the molecules at any given temperature is inversely related to the mass of the molecules with lighter molecules being faster. So let's take a look at the mass of the candidate molecules and see which is lighter and therefore faster. CH4 - Molar mass is about 16. CO - Molar mass is about 28 Ar - Molar mass is about 40 CO2 - Molar mass is about 44 If the 4 options, CH4 (methane) is by far the lightest, and therefore the fastest, so will effuse faster than the other 3 gasses.</span>

____ [38]2 years ago

5 0

I think CO2 because its something common LMFOA

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A rock sample has a mass of 16 grams and a volume

MAVERICK [17]

Answer:

128

Explanation:

because you multiply them

8 0

3 years ago

The main constituent of gallstones is cholesterol. Cholesterol may have a role in heart attacks and blood clot formation. Its el

Nataly [62]

The main constituent of gallstones is cholesterol. Cholesterol may have a role in heart attacks and blood clot formation. Its elemental percentage composition is 83.87% C, 11.99% H, and 4.14% O. It has a molecular weight of 386.64 amu. Empirical formula is C₃H₄O₁ and Molecular formula is 7(C₃H₄O₁).

<h3>What is Empirical Formula ?</h3>

Empirical formula is the simplest whole number ratio of atoms present in given compound.

Element % Atomic mass Relative no. of atoms Simplest whole ratio

C 83.87 12 $\frac{83.87}{12}$ = 6.98 $\frac{6.98}{0.25}$ = 3

H 11.99 1 $\frac{11.99}{1}$ = 11.09 $\frac{11.09}{0.25}$ = 4

O 4.14 16 $\frac{4.14}{16}$ = 0.25 $\frac{0.25}{0.25}$ = 1

Thus the empirical formula is C₃H₄O₁.

<h3>How to find the Molecular formula of compound ?</h3>

Molecular formula = Empirical formula × n

n = $\frac{\text{Molecular weight}}{\text{Empirical formula weight}}$

= $\frac{386.64}{56}$

= 7

Molecular formula = Empirical formula × n

= 7 (C₃H₄O₁)

Thus from the above conclusion we can say that The main constituent of gallstones is cholesterol. Cholesterol may have a role in heart attacks and blood clot formation. Its elemental percentage composition is 83.87% C, 11.99% H, and 4.14% O. It has a molecular weight of 386.64 amu. Empirical formula is C₃H₄O₁ and Molecular formula is 7(C₃H₄O₁).

Learn more about the Empirical Formula here: brainly.com/question/1603500

#SPJ4

7 0

2 years ago

1. When the temperature of a rigid hollow sphere containing 685 L of helium gas is

mote1985 [20]

<h3>Answer:</h3>

250.756 moles He

<h3>Explanation:</h3>

From the question we are given;

Volume, L = 685 L

Temperature, T = 621 K

Pressure, P = 189 × 10 kPa

We are required to calculate the number of moles of the gas,

Using the Ideal gas equation,

PV = nRT, where P is the pressure, V is the volume, T is the temperature, n is the number of moles, and R is the ideal gas constant.

We can replace the known variables and constant in the equation to get the unknown variable, n.

Using ideal gas constant as 8.3145 L.kPa/K/mol

$n=\frac{PV}{RT}$

$n=\frac{(1890)(685)}{(8.3145)(621)}$

$n = 250.7557 moles$

n = 250.756 moles

The moles of helium contained in the sphere is 250.756 moles

6 0

2 years ago

Which of the following elements are good insulators?

ale4655 [162]

P and S
___________________________________________________________

6 0

2 years ago

Read 2 more answers

a cylinder rod formed from silicon is 46.0 cm long and has a mass of 3.00 kg. the density of silicon is 2.33 g/cm³. what is the

Gnesinka [82]

$d=\frac{m}{V}\\\\
V=\pi r^{2}H\\$ $d=\frac{m}{\pi r^{2}H} \ \ \ |*\pi r^{2}H\\\\
d \pi r^{2}H=m \ \ \ |:d \pi H\\\\
r^{2}=\frac{m}{d \pi H}\\\\
r=\sqrt{\frac{m}{d \pi H}}\\\\
2r=d\\\\
d=2\sqrt{\frac{m}{d \pi H}}$

$H=43cm\\
d=2.33\frac{g}{cm^{3}}\\
m=3kg=3000g\\\\
d=2\sqrt{\frac{m}{d \pi H}}=2*\sqrt{\frac{3000g}{2.33\frac{g}{cm^{3}} * \pi * 43cm}}=2*\sqrt{\frac{3000}{100,19\pi \frac{1}{cm^{2}}}}\approx6,17cm$

7 0

2 years ago