321 Answered Questions for the topic Chemistry Lab

Chemistry Lab

05/01/16

What is the solubility of sugar and numerical value? Why did the sugar attach to the skewer?
I am making rocky candy for a lab in chemistry and have a couple of problems I am stuck on.    1. Why did the sugar leave the solution and attach to the stick?    2. What is the solubility of... more
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Chemistry Lab Chemistry

04/28/16

lab report help, 53.3 g/mol is ethanol or propanol
we did a lab, i got 53.3 g/mol as the molar mass for the result, it can either be ethanol or propanol, which is better. propanol is closer, but it is a lab, so it isnt an accurate result in the... more
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04/10/16

Ksp and the Common Ion Effect
I just completed a lab in which I titrated Calcium Iodate with Na2S2O3. During the titration we were told to add a starch once the liquid had turned light yellow. When we did this it became dark... more
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04/10/16

2 Redox titration questions??? Please help!!! General Chemistry Lab?
Q1. Iron is often used to standardize permanganate solutions. A 0.158 g sample of pure iron wire was dissolved in dilute sulfuric acid to form a solution of iron (II) sulfate. This was titrated... more
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04/10/16

Redox titration question? Determine the molarity of a solution? PLEASE HELP!!
Q1. Iron is often used to standardize permanganate solutions. A 0.158 g sample of pure iron wire was dissolved in dilute sulfuric acid to form a solution of iron (II) sulfate. This was titrated... more
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Chemistry Lab Molar Mass

03/20/16

chem helo plss
starting with n=g/MM and PV=nRT, detrive the formula for molar mass
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Chemistry Lab

03/19/16

What are the sources of error for the combustion of acetylene gas
 4 test tubes have been filled with different amounts of acetylene. One completly full , half full and so on. The one with less acetylene produced a complete combustion. What are the sources of... more
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Chemistry Lab Chemistry Moles Equilibrium

03/16/16

How do I work out the molarity and equilibrium constant using moles of reactants?
The equation is C2H5OH(aq) + CH3CO2H(aq) ? CH3CO2C2H5(aq) + H2O(l)   Moles of ethanol: 0.0747 Moles of ethanoic acid: 0.0112   amount of ethanol used in experiment: 4cm3 amount of ethanoic... more
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Chemistry Lab

03/16/16

describe the relationship between surface tension and intermolecular forces of attraction found among the pure water sample versus the water-detergent mixture
 hydrogen bonding in water lab
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03/16/16

A student heats magnesium to produce magnesium oxide.
A student heats magnesium to produce magnesium oxide. the reaction is below:Mg + O2 MgOShe starts wih 3.45 grams of magnesium and produces 5.65 grams of magnesium oxide. Calculate her theoretical... more
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03/16/16

A student calculates the theoretical yield of their experiment is 4.89 grams
A student calculates the theoretical yield of their experiment is 4.89 grams. After carrying out the experiment, they only produced 4.21 grams of product in the lab. Calculate the percent yield... more
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03/16/16

Chemistry Problem:stoichiometry
 Al+S8 -->Al2S3-How many moles of aluminum are required to produce 56.9 grams of sulfur?-5.0 grams of aluminum sulfide is needed. How many grams of sulfur is required to make it?
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03/15/16

What is the theoretical yield of CuO?
What is the theoretical yield of CuO? -Experimental yield of Copper II oxide-1.4-Equation-CuCO3.Cu(OH)2 -->CuO + CO2+H2O
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Chemistry Lab

03/14/16

Some people store their batteries in the freezer to help them last longer. Using two different theories explain the chemistry behind this thought process
Some people store their batteries in the freezer to help them last longer. Using two different theories explain the chemistry behind this thought process.
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03/14/16

What is the theoretical yield of CuO?
What is the theoretical yield of CuO?   -Experimental yield of Copper II oxide-1.4 -Equation-CuCO3.Cu(OH)2 -->CuO + CO2+H2O
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03/11/16

Stoichiometry Lab
CuCO3.Cu(OH)2--> CO2+H2O+2CuO How many grams of Copper II oxide are produced if you start with 1.01 g of Copper II carbonate.
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03/10/16

Stoichiometry Problem
C2H4 + O2 → CO2 + H2O -If you start with 45 grams of ethylene (C2H4), how many grams of carbon dioxide should be produced?-Theoretically, how many liters of carbon dioxide will you produce if 55.3... more
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Chemistry Lab Chemistry

03/09/16

If you need to prepare 5 g of sodium chloride how many mililiters of 2 M hydrochloric acid do you need to measure?
This is the formula : NaHCO3 + HCl = NaCl + CO2 + H2O
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Chemistry Lab Chemistry Moles Liters

03/05/16

If I wanted to dilute a 6.2 L, 3M NaNO3 solution to make a 4.7M NaNO3 solution....
How many L of NaNO3 would I need to add?
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Chemistry Lab

03/04/16

Empirical formula question
Please help me, thank you.   Magnesium ions have a charge of +2 while oxygen ions have a charge of -2. Considering these charges, what is the empirical formula of magnesium oxide ?
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Chemistry Lab Chemistry Percentages Mass

03/02/16

Separating mixtures in chemistry lab (PLEASE HELP. URGENT!)
You are to separate the two components of a mixture of sand and sugar. The initial mass of the mixture is 32.4563g. You found that the mass of sand was 19.5642g.    A) Describe the procedure you... more
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Chemistry Lab

02/24/16

4NH3+5O2->4NO+6H2O
If the results from the lab actually produced 9.2 grams of H2O, then what was the percent yield?
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Chemistry Lab Chemistry

02/22/16

How many grams of CuSO4*5H20 are needed to prepare a 0.020 M stock solution?
I'm in General Chemistry in college and just need the answer to this question. It'd be really cool if you could show/explain how to do this if you can. That would be a huge help. Thanks for your time. more
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Chemistry Lab

02/19/16

Substances and their changes
When natural gas is burned in the laboratory burner, does the gas undergo a physical change or does it undergo a chemical change? Explain
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Chemistry Lab Chemistry Mass Gold Density

02/18/16

Gold Density Question. IMPORTANT! NEED BY TOMORROW
A "pure gold" bracelet has a mass of 105.36 grams. When placed in a graduated cylinder which you read to contain 25.5 mL of water, the water level rises to read 32.0 mL. Find the density of pure... more
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