Which of the following represents the mass of 1 molecule of sh2?

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Which of the following represents the mass of 1 molecule of sh2?

5.645 × 10⁻²³ g

Solution:

Step 1) Calculate Molar Mass of SH₂;

Atomic Mass of Sulfur = 32 g/mol

Atomic Mass of H₂ = 2 g/mol

Molecular Mass of SH₂ = 34 g/mol

Step 2: Calculate mass of one molecule of SH₂ as;

As,

Moles = # of Molecules / 6.022 × 10²³

Also, Moles = Mass / M.Mass So,

Mass/M.mass = # of Molecules / 6.022 × 10²³

Solving for Mass,

Mass = # of Molecules × M.mass / 6.022 × 10²³

Putting values,

Mass = (1 Molecule × 34 g.mol⁻¹) ÷ 6.022 × 10²³

Mass = 5.645 × 10⁻²³ g

a) A = 4.0 m , b) w = 3.0 rad / s , c) f = 0.477 Hz , d) T = 20.94 s

Explanation:

The equation that describes the oscillatory motion is

x = A cos (wt + fi)

In the exercise we are told that the expression is

x = 4.0 cos (3.0 t + 0.10)

let's answer the different questions

a) the amplitude is

A = 4.0 m

b) the frequency or angular velocity

w = 3.0 rad / s

c) angular velocity and frequency are related

w = 2π f

f = w / 2π

f = 3 / 2π

f = 0.477 Hz

d) the period

frequency and period are related

T = 1 / f

T = 1 / 0.477

T = 20.94 s

e) the phase constant

Ф = 0.10 rad

f) velocity is defined by

v = dx / dt

v = - A w sin (wt + Ф)

speed is maximum when sine is + -1

v = A w

v = 4 3

v = 12 m / s

g) the angular velocity is

w² = k / m

k = m w²

k = 1.2 3²

k = 10.8 N / m

h) the total energy of the oscillator is

Em = ½ k A²

Em = ½ 10.8 4²

Em = 43.2 J

i) the potential energy is

Ke = ½ k x²

for t = 0 x = 4 cos (0 + 0.1)

x = 3.98 m

j) kinetic energy

K = ½ m v²

for t = 00.1 ²

v = A w sin 0.10

v = 4 3 sin 0.10

v = 1.98 m / s

34.1amu

Explanation:

1) A. 0.0515 L

2) B. 35.504 L

3) B. 422.446 g

Explanation:

At STP, you have 0.101 g of carbon dioxide gas. What is the volume of this gas?

Step 1: Data given

Mass of CO2 gas = 0.101 grams

Molar mass of CO2 = 44.01 g/mol

STP = 1 atm and 273K

Step 2: Calculate moles CO2

Moles CO2 = mass CO2 / molar mass CO2

Moles CO2 = 0.101 grams / 44.01 g/mol

Moles CO2 = 0.0023 moles

Step 3: Calculate the volume

For 1 mol at STP we have 22.4L

0.0023 moles we have 22.4L * 0.0023 = 0.0515 L

Option A is correct

You have 27g of ammonia (nitrogen trihydride) at STP. What is the volume? Hint...you will first need to convert mass of ammonia to moles!

Step 1: Data given

Molar mass of NH3 = 17.03 g/mol

Mass of NH3 = 27.00 grams

STP = 1 atm and 273K

Step 2: Calculate moles NH3

Moles NH3 = 27.00 grams / 17.02 g/mol

Moles NH3 = 1.585 moles

Step 3: Calculate volume

For 1 mol at STP we have 22.4 L

For 1.585 moles we have 22.4 * 1.585 = 35.504 L

Option B is correct

Which of the following represents the MASS of 215 L of dinitrogen monoxide at STP? Hint...find the # of moles of this gas and then use the molar mass to go from moles to mass!

Step 1: Data given

Volume = 215 L

STP = 1 atm and 273 K

Molar mass of N2O = 44.01 g/mol

Step 2: Calulate moles N2O

22.4L = 1 mol at STP

215 L = 215 / 22.4 = 9.60 moles

Step 3: Calculate mass N2O

Mass N2O = moles N2O * molar mass N2O

Mass N2O = 9.60 moles* 44.01 g/mol

Mass N2O = 422.446 g

Option B is correct

The answer is D. An oxygen molecule, O2 (because oxygen's natural state is diatomic), consists of two oxygen atoms. You would calculate the mass of a mole of oxygen molecules as 16.00 * 2 grams. To find the mass of one molecule, use the conversion factor 1 mole / 6.02e23 molecules. The mass of one oxygen molecule would then be 16.00 * 2 / 6.02e23