Calculate the mass in grams of each of the following...

Calculate the mass in grams of each of the following samples. a. 0.000471 mol of carbon monoxide b. $1.75 \times 10^{-6}$ mol of gold(III) chloride c. 228 mol of iron(III) chloride d. 2.98 millimol of potassium phosphate (1 millimol = 1/1000 mol) e. $2.71 \times 10^{-3}$ mol of lithium chloride f. 6.55 mol of ammonia

Calculate the mass in grams of each of the following samples.
a. 0.000471 mol of carbon monoxide
b. $1.75 \times 10^{-6}$ mol of gold(III) chloride
c. 228 mol of iron(III) chloride
d. 2.98 millimol of potassium phosphate (1 millimol = 1/1000 mol)
e. $2.71 \times 10^{-3}$ mol of lithium chloride
f. 6.55 mol of ammonia

Key Concepts

Mole Concept

The concept of the mole is a fundamental principle in chemistry that represents a specific number of particles (such as atoms, molecules, or ions), which is approximately 6.022 x 10^23 particles. It provides a bridge between the atomic scale and the macroscopic quantities of material, allowing chemists to count entities in a sample by weighing it.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms present in the chemical formula of a compound. This value is crucial for converting between the mass of a substance and the amount in moles.

Mass-to-Mole Conversion

The conversion from moles to grams is performed using the formula 'mass = number of moles × molar mass'. This relationship allows one to determine the mass of a substance when the amount in moles is known, which is essential for preparing solutions, balancing reactions, and performing quantitative analyses in chemistry.

Unit Conversion

Unit conversion is an important aspect when dealing with different scales or units in chemical calculations, such as converting millimoles to moles. Proper handling of units ensures that mathematical operations are consistent and that the final results are expressed in the desired units, such as grams in this case.

Transcript

00:01 So in this example you have to calculate the mass from the moles.

00:05 A they have given 6 .14 into 10 to minus 4 moles of so3, then b 3 .11 into 10 to 5 moles of lead oxide, then c .495 moles of cscl3, then d 2 .45 into 10 to a minus 8 moles of a trichlorated, then e .167 mole of a lrh and f 5 .266 moles of a copper.

00:30 Fluoride.

00:31 So let us begin with this exercise.

00:33 So you know they are given 6 .14 into 10 to minus 4 moles of so3.

00:44 M so you have to use the formula n is equal to w upon yam and therefore w is equal to n into m therefore yon is 6 .14 into 10 to minus 4 into to molar mass of sulfolite oxide it is 80, 80 and that is equal to 491 .2 into 10 -h -2 minus 4, okay and therefore mass in grams of grams of 6 .14 into 10 -h -2 minus 4 moles of so3 that is equal to 4 .912 into 10 dash 2 minus 2 grams.

01:48 So this one the answer.

01:56 Then second one 3 .11 into 10 dash to 5 moles of pbo.

02:20 Now once again, n is equal to w upon yam and therefore w is equal to n is equal to n n into m and that is equal to yin is 3 .11 into 10 dash to 5 into molar mass of lead oxide it is 223 .2 that is equal to 694 .152 into 10 dash to 5 and therefore answer is that is mass n gram of 3.

03:00 11 .10 .10 .10 .5 moles of pbo that is equal to 6 .94152 into 10 dash to 7 grams.

03:30 The next c1 that is 0 .495 moles of chloroform.

03:50 Now you know w is equal to n into m therefore w is equal to 0 .495 into 119 .38 and therefore w is equal to mass in gram of mass in gram of 0 .45 of 0 .45 moles of chloroform that is equal to 59 .0 .031 gram...

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