Number of results: 39,267
how do i figure out the percentage error , as well as the absolute error of a) (10.00+/- .02)mL x .42 mol/L b) (10.00 +/- .02)mL + (10.00 +/- .02)mL
Friday, January 16, 2009 at 1:26am by eddie
http://science.widener.edu/svb/stats/error.html On the first, percent error is .02/10 x 100 absolute error is .02 On the last, you have to do some math. See the link error=sqrt (.02^2+ .02^2)=.028 then, use the formulas above.
Friday, January 16, 2009 at 1:26am by bobpursley
college chem. please help!!
Calculate the % empty space in 1 mole of water at 25 degree C (d=0.9971g/ml). The volume of a water molecule can be taken as the sum of the volumes of the 2 hydrogen molecules and the oxygen atom. Use the single bonded covalent radii of 37pm for hydrogen and 66pm for oxygen.
Tuesday, February 3, 2009 at 9:54pm by christy
Calculate the total number of electrons that can be present in the principal level for which n = 4.
Wednesday, April 15, 2009 at 4:07pm by Justyna
Number of electrons possible in N is 2N^2 so 2*4^2 = ??
Wednesday, April 15, 2009 at 4:07pm by DrBob222
Two questions where I have to write a balanced net ionic equation. 1. Write a balanced net ionic equation for the reaction that occurs when aqueous solutions of sodium chromate and silver nitrate are mixed 2. Write a balanced net ionic equaion reaction for the acid-base ...
Tuesday, June 2, 2009 at 7:05pm by kelly
how many milliliters of 0.200 M Na2S2O3 are needed to provide 0.0388 mol Na2S2O3?
Tuesday, June 2, 2009 at 7:06pm by kelly
how many grams of NH4Cl are required to prepare 250 mL of .122 M NH4Cl solution? I set this up using the molarity equation and the part that I was missing is moles. So I divided the 0.122 by .25 L and got .031 mol. Then I took that and multiplied it by the molar mass of NH4Cl ...
Tuesday, June 2, 2009 at 7:09pm by kelly
What you did looks ok to me. 1.72 g?It could be that you rounded the 0.0305 to 0.031 too soon. You are allowed three significant figures so I would use 0.0305 for the moles required.
Tuesday, June 2, 2009 at 7:09pm by DrBob222
M x L = moles.
Tuesday, June 2, 2009 at 7:06pm by DrBob222
For net ionic equations. 1. Write the molecular equation. 2. Separate into ions everything EXCEPT a. insoluble materials. b. gases. c. weak electrolytes. For everything in 2, write them as the molecule. Have a try at these and I'll be glad to check them for you.
Tuesday, June 2, 2009 at 7:05pm by DrBob222
In this experiment a hot metal block at 100oC is added to cold water in a calorimeter. The heat lost by the metal block equals the heat gained by the water and the two end up at the same temperature. In one experiment, the mass of the metal block is 89.5 grams, the volume of ...
Thursday, October 8, 2009 at 4:30pm by Sarah
mass metal x specific heat metal x (Tfinal-Tinitial) + mass water x specific heat water x (Tfinal-Tinitial) = 0 You can pick out the pieces you want from above to answer your questions. For Dulong and Petit. heat capacity = about 24.9 J/mol*K. (about 6.3 calories/g*C
Thursday, October 8, 2009 at 4:30pm by DrBob222
calculate the density of O2 gas( in g/L) at 1.22 atm and 25 degrees C
Wednesday, November 11, 2009 at 9:05pm by amanda
Use PV = nRT. Calculate n, number of moles. n x molar mass = grams. If you plugged in 1.00 L for the volume, then g/L will be the density.
Wednesday, November 11, 2009 at 9:05pm by DrBob222
I have finals coming up in a week and a half. I know I should have started studying earlier, but I just had an exam in my chem class and was focused on getting the information for that exam mastered before I started studying for the final. Now, I'm overwhelmed. I have no idea ...
Monday, November 30, 2009 at 7:16pm by Katherine
homework college chem.
a sample of gas occupies a volume at 73. 1 mL. As it expands, it does 135.0 J of work on its surroundings at a constant pressure of 783 torr. what is the final volume of gas?
Sunday, February 26, 2012 at 12:58am by danielle
College Chem 1010
Here is a simplified list of solubility rules. http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html A) Ca(NO3)2 B) FePO4 C) NH4OH D) Na2SO4 E) NaCl
Sunday, April 15, 2012 at 10:48pm by DrBob222
Tuesday, June 26, 2012 at 1:36am by bobpursley
homework college chem.
w= -PΔV -135.0 J = -783 torr × (Vfinal - 73.1 mL) -1350 J × (1L atm)/(101.32 J) = -783 torr × (1atm/760 torr) × (Vfinal -73.1 ml × 1L/1000 mL) Vfinal= (-1350 J × (1 L atm)/(101.32 J))/(-783 torr × (1 atm)/(760 torr)) + 73.1 mL × (1L/1000 mL) = 1.36 L Vfinal = 1.36 × (...
Sunday, February 26, 2012 at 12:58am by Chelsea N