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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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When heated, solid copper(II) carbonate decomposes to solid copper(II) oxide and carbon dioxide gas. What is the chemical equation (including phases) that describes this reaction?
This reaction is balanced with respect to mass and charge; as indeed it must be if it reflects chemical reality. Most carbonates undergo this decomposition, provided you supply enuff heat...
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I measured $"5.00 g"$ copper sulfate solid and $"6.530 g"$ zinc. If for this reaction $q_(rxn) = "979.72 cal"$ of energy was involved, why is my percent error of the standard enthalpy of reaction for the reaction of zinc with copper sulfate so big???
Based on the information I got from you: $m_"Zn" = "6.530 g"$ $m_("CuSO"_4cdot5"H"_2"O") = "5.00 g"$ (in lab you tend to be handed the hydrate) From the molar...
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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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A bottle of calcium bromide contains a bromide ion concentration of 0.10 mol/L. What is the concentration of the calcium bromide?
Calcium bromide speciates in aqueous solution according to the following equation......... $CaBr_2(s) stackrel(H_2O)rarrCa^(2+) + 2Br^-$ And thus for every metal ion there are necessarily two bromide ions. Here by...
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How can I solve this ??
dentify the electrolyte solution with the largest concentration of ions.
A. 1.0 moles KOH in 2.0 L water
B. 1.0 moles AlCl3 in 2.0 L water
C. 1.3 moles MgCl2 in 3.0 L water
D. 1.5 moles NaCl in 4.0 L water
will generally dissociate into ions in solution. For the purposes of this problem, let's assume there isn't much ion pairing. The key here is knowing we're worried about...
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Sea water contains $65 xx10^-3$ $"g/L"$ of bromide ions. If all the bromide ions are converted to produce $Br_2$,how much sea water is needed to prepare 1 kg of $Br_2$?
please tell the method.
We know that the sea water contains $(65xx10^-3"g of bromide ions")/L $ If you want $Br_2$ the following reaction takes place $Br^-) + Br^-) = Br_2 + 2e^-$ Well this...
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In the reaction of aluminum bromide with ionized sodium bromide, which compound is the Lewis acid?
The Lewis concept of acidity designates acids as electron pair acceptors, and bases as electron pair donors. For the reaction: $AlBr_3 + Br^(-) rarr AlBr_4^-$, clearly the bromide ion is...
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