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A mass of mercury occupies 0.95 L. What volume would an equal mass of ethanol occupy? The density of mercury is 13.546 g/mL and the density of ethanol is .789 g/mL?
For a given substance, its tells you the mass occupied by one unit of volume of that substance. In essence, is a measure of how well the molecules of...
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A copper penny has a mass of $3.1$ $g$ and a volume of $.35$ $cm^3$. What is the density of copper?
$"Density"$ $=$ $"Mass"/"Volume"$ by definition. Now this is the of the copper coin, not copper. In the UK copper coins, the $1$ $p$ and $2$ $p$ coins are copper plated...
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If the density of and object is 4.0 g/cm3 and the mass is 4.0kg then how mach volume does the object occupy? Could you also show how you got there?
Alright so we know the formula for is $rho=m/v$ => where $rho$ is the density with units of the derived components, $m$ is the mass, and $v$ is the volume....
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You have 48.3g of solid lithium sulfate. If it has a density of $"2220 g/L"$, what volume will this solid occupy?
The problem tells you that lithium sulfate has a of $color(blue)("2220 g")$ $color(purple)("L"^(-1))$, which means that every $color(purple)("1 L")$ of lithium sulfate has a mass of $color(blue)("2220 g")$. In your...
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A graduated cylinder is filled with water to a level of 40.0 ml. When a piece of copper is lowered into the cylinder, the water level rises to 63.4 mL. What is the volume of the copper sample? If the density of the copper is 8.9 g/cm^, what is its mass?
Do you agree? The copper displaces the given volume of water. Now $rho_"Cu"=8.90*g*cm^3$ OR $rho_"Cu"=8.90*g*mL^-1$, i.e. $1*mL-=1*cm^3$ But by definition, $rho_"density"="mass"/"volume"$ And thus $"mass"=rhoxx"volume"=8.90*g*cancel(mL^-1)xx23.4*cancel(mL)$ $=208.3*g$. Do you follow?
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Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: $Cu_2S(s) + O_2(g) -> 2Cu(s) + SO_2(g)$. What mass of copper(I) sulfide is required in order to prepare 0.650 kg of copper metal?
You have given the stoichiometric equation that represents reduction of cuprous sulfide: $Cu_2S(s) + O_2(g) rarr 2Cu(s) + SO_2(g)$ Sulfur is oxidized; copper and oxygen are reduced. $"Moles of copper"=(650*g)/(63.55*g*mol^-1)=10.3*mol$....
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A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. How can a sample of copper chloride crystals be made from copper carbonate and dilute hydrochloric acid?
$CuCO_3(s) + 2HCl(aq)rarrCuCl_2(aq) + CO_2(g)uarr + H_2O(l)$ Or........... $CuO(s) + 2HCl(aq)rarrCuCl_2(aq) + H_2O(l)$ For each acid base reaction the product is the beautiful blue-coloured $[Cu(OH_2)_6]^(2+)$ ion, which is commonly represented...
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Hydrogen was passed over heated 2g copper oxide till only copper was left. The mass of copper obtained was was 1.6 grams. What is the percentage of oxygen in copper oxide?
There is a loss of 0.4 grams. $ 2.0 -1.6$ = 0.4 grams $ 0.4/2.0 xx 100 $ = 20% The Hydrogen will combine with the Oxygen in...
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Copper will react with sulfur to form a copper sulfide, if 1.500g copper reacts with sulfur to form 1.880g of copper sulfide, what is the empirical formula of the copper sulfide?
The idea here is that you need to use the mass of copper and the mass of the copper sulfide to determine how much sulfur the produced compound contains, then...
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An oxide of copper contains 2.118 g of copper and 0.2666 g of oxygen. Another oxide of copper contains the same mass of copper but 0.5332 g of copper. What are the empirical formulas of the oxides?
The empirical formulas are $"Cu"_2"O"$ and $"CuO"$. Oxide 1 $color(white)(mmmmml)"Cu" +color(white)(m) "O" → "Oxide 1"$ $"Mass/g":color(white)(l) 2.118color(white)(ll) 0.2666$ Our job is to calculate the ratio of the moles of...
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