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The density of pure gold is $19.3$ $g$$/$$cm^3$. What is the mass of a nugget that has a volume of $1.47$ $cm^3$?
$19.3 g/cancel(cm^3)*1.47cancel(cm^3)~~28.4g$
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Calculate the mass density of a pure sample of oxygen gas at a pressure
of 1.0 atm, a volume of 7.8 L at 197.2C?
We can use the to solve this problem. $color(blue)(|bar(ul(color(white)(a/a)PV = nRT color(white)(a/a)|)))" "$ Since $"moles" = "mass"/"molar mass"$ or $n = m/M$, we can write $PV...
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Natasha's mother gave her a solid gold necklace. She determines the chain has a mass of $7.6$ $g$. The density of pure gold is $19.3$ $g$$/$$cm^3$. About how much gold was used to make her necklace?
Assuming that the neckless is made from $"24K"$, $24$ karat gold, i. e. gold that is $99.9%$ pure, you can solve this problem by using the mass of the neckless...
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Archermedes was commissioned to determine if the crown given to the king was pure gold or not. If the crown had a mass of 882 grams and displaced 50.0 mL of water, was the crown pure gold?
Gold has a , $rho=19.3*g*mL^-1,$ which is approx. 20 times as much water. The density of the gold crown (given to the tyrant of Syracuse, not the king), was...
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Glycerol is a syrupy liquid often used in cosmetics and soaps. A 2.50-L sample of pure glycerol has a mass of 3.15 x 10^3 g. What is the density of glycerol in grams per cubic centimeter?
$"Density, "rho$ $-=$ $"Unit mass"/"Unit Volume"$ Here, both mass and volume were quoted, and we simply take the quotient, knowing that $1*L$ $=$ $1000*cm^3$. Thus $"rho$ $-=$ $(3.15xx10^3g)/(2.50*cancelLxx10^3*cm^3*cancel(L^-1))$ $=$ $??g*cm^-3$
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The density of a material is 5.0 g/cm^3. If a sample of pure silver has a volume of 2 mL, what is the mass in kg?
$"Density"$ $=$ $"Mass"/"Volume"$ I have an idea that the of silver metal is greater than $10.0*g*mL^-1$ (this is typical of the heavier metals!). You will have to look this up...
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A gold colored ring has a mass of 18.9 grams and a volume of 1.12 mL. Is the ring pure gold?
d = $m/v$ First fill in the m and v $(18.9g)/(1.12mL)$ Then, divide $(18.9g)/(1.12mL) = 16.88 g//mL$ Thus, making the ring not pure.
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How would you define pure substance? What are some examples of pure substances?
A pure substance has definite physical and chemical properties....which include melting point, boiling point, (under given conditions),......... And examples of pure substances include all the , water, methane gas, sugar,...
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What is the atomic mass of hafnium if, out of every 100 atoms, 5 have a mass of 176, 19 have a mass of 177, 27 have mass of 178, 14 have a mass of 179, and 35 have a mass of a 180?
If there are two an element $"Average atomic mass" = "mass"_axx "fract"_a + "mass"_b xx "fract"_b$ In the given problem about Hafnium, 5 isotopes have been given. Extending the...
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What is the average atomic mass of an element if, out of 100 atoms, 5 have a mass of 176 amu, 19 have a mass of 177 amu, 27 have a mass of 178 amu, 14 have a mass of 179 amu, and 35 have a mass of 180 amu?
The $"Average Atomic Mass"$ of an element is defined as "the weighted average mass of all naturally-occurring (occasionally radioactive) of the element." (and hence the name "average") [1] Dividing the...
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