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3 years ago

How many atoms are in 0.625 moles of ge (atomic mass = 72.59 amu)?

Chemistry

2 answers:

lord [1]3 years ago

8 0

0.625 moles of ge X 6.02x10^23 atoms/ 1 mol of ge equal to 3.76x10^23 atoms of ge, just times with Avogadro.

Vikki [24]3 years ago

8 0

Answer:

3.76 × 10²³ atoms

Explanation:

1 mole = 6.022 × 10²³ atoms (Avogadro's number)

Therefore, 0.625 moles of Ge will have:

Multiply the given moles by number of atoms per mole.

= 0.625 moles ×6.022 × 10²³ atoms/mol

= 3.76 × 10²³ atoms

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Why is it difficult to accurately represent ammonia and methane on paper?

andrew-mc [135]

Answer:

The correct answer is because the molecular structure.

Explanation:

The difficulty of ammonia and methane to be represented on paper is due to the molecular structure. These compounds have a three-dimensional projection with defined angles. Ammonia presents angles of 109.5º between the atom of Nitrogen and those of Oxygen. The ammonia presents 107.8º between the oxygen atoms.

In the methane molecule, there is 109.5º between the hydrogen molecules and the carbon atom. This results in the need for a 3D representation of the molecule.

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3 years ago

How would you calculate the molar mass of 2AgCl?

Rashid [163]

2 × (atomic mass of Ag) + (atomic mass of Cl (

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3 years ago

A 17.4 L sample of oxygen gas (O2) was collected at a temperature of 23.0°C and a pressure of 2.18 atmospheres. What volume woul

timofeeve [1]

The volume of the gas at STP = 35.01 L

<h3>Further explanation</h3>

Conditions at T 0 ° C and P 1 atm are stated by STP (Standard Temperature and Pressure).

In general, the gas equation can be written

$\large {\boxed {\bold {PV = nRT}}}$

where

P = pressure, atm

V = volume, liter

n = number of moles

R = gas constant = 0.08206 L.atm / mol K

T = temperature, Kelvin

V=17.4 L

T = 23 + 273 = 296 K

P = 2.18 atm

$\tt mol=n=\dfrac{PV}{RT}\\\\n=\dfrac{2.18\times 17.4}{0.082\times 296}\\\\n=1.563$

The volume of the gas occupy at STP :

$\tt 1.563\times 22.4=35.01~L$

6 0

3 years ago

A 5.024 mg sample of an unknown organic molecule containing carbon, hydrogen, and nitrogen only was burned and yielded 13.90 mg

Dafna1 [17]

Answer:

C8H17N

Explanation:

Mass of the unknown compound = 5.024 mg

Mass of CO2 = 13.90 mg

Mass of H2O = 6.048 mg

Next, we shall determine the mass of carbon, hydrogen and nitrogen present in the compound. This is illustrated below:

For carbon, C:

Molar mass of CO2 = 12 + (2x16) = 44g/mol

Mass of C = 12/44 x 13.90 = 3.791 mg

For hydrogen, H:

Molar mass of H2O = (2x1) + 16 = 18g/mol

Mass of H = 2/18 x 6.048 = 0.672 mg

For nitrogen, N:

Mass N = mass of unknown – (mass of C + mass of H)

Mass of N = 5.024 – (3.791 + 0.672)

Mass of N = 0.561 mg

Now, we can obtain the empirical formula for the compound as follow:

C = 3.791 mg

H = 0.672 mg

N = 0.561 mg

Divide each by their molar mass

C = 3.791 / 12 = 0.316

H = 0.672 / 1 = 0.672

N = 0.561 / 14 = 0.040

Divide by the smallest

C = 0.316 / 0.04 = 8

H = 0.672 / 0.04 = 17

N = 0.040 / 0.04 = 1

Therefore, the empirical formula for the compound is C8H17N

8 0

3 years ago

.......state Hess law

alexgriva [62]

Hess's Law of Constant Heat Summation (or just Hess's Law) states that regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes. This law is a manifestation that enthalpy is a state function.

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3 years ago