mass of mg- .28 mass of o- .41 calculate the moles of mg and o what is the simples whole number ratio of the moles of mg to the moles of o? round off to the nearest whole number ratio

60,113 results
  1. Chem

    Plese tell me if these are right. A 15.0-mL sample of NaCl solution has a mass of 15.78g. After the NaCl is evaporated to dryness, the dry salt residue has a mass of 3.26g. Calculate the following concentrations for the NaCl solution. a. %(m/m)= 3.26 x 100

  2. Chem 11

    So I did a lab determining the chemical formula of a hydrate. I really just need somebody to check this over for me. We had to find the molecular formula of a hydrate of copper (2) sulphate, CuSO4 .xH2O. My observation table looks like this: Mass of clean,

  3. Chemistry

    Many metals react with oxygen gas to form the metal oxide. For example calcium reacts: 2Ca(s) + O2(g)--> 2CaO(s) Calculate the mass of calcium prepared from 4,20g of Ca and 2.80g of O2. (a) How many moles of CaO can form from the given mass of Ca? (b) How

  4. chemistry

    8.What is the mass of 4.56 moles of sulfur dioxide? 9.What is the mass of 4.56 molecules of sulfur dioxide? 10.How many formula units are in 0.456 grams of Ca3(PO4)2? 11.How many moles are in 1.5 x 10 ^23 atoms of fluorine? 12.What is the mass of 2.80 x 10

  5. chemistry

    mass of crucible- 26.4574g mass of crucible and hydrated sample- 27.7617g mass of hydrated sample 1.3043g mass of crucible and dehydrated sample- 27.5693g mass of dehydrated sample- 1.1119g mass of filter paper- 0.7089g mass of filter paper and copper-

  6. Chemistry

    I am completing my lab and cannot figure this out. I need someone to go over it and make sure I am right because I can't figure out why my empirical formula does not match the molecular formula. #7 is the one I am really having a problem with, but here is

  7. General Chemistry

    The formula of a compound of lead (Pb) and sulfur (S) was determined using the method in this module. A sample of Pb was weighed into a crucible and covered with finely powdered S. The crucible was covered and heated to allow the Pb and S to react.

  8. Physics AP

    A conical pendulum is formed by attaching a 50 g mass to a 1.2m string. The mass swings around a circle of radius 25cm. A claculate the speed of the mass. B Calculate the acceleration of the mass. C calculate the tension in the string

  9. chemistry

    Calculate the weight (in mg) of borax Na2B4O7.10H20 required to react with 25.0 mL if 0.100 M HCI No. moles HCl consumed = __________ moles No. moles borax required = __________ moles Molar mass of borax = __________ g mol-1 (Na2B4O7.10H2O) Weight borax

  10. Chem (Help!)

    I really need help answering these questions. A sample of CO2 gas with a mass of 0.30 g is placed in a 250 mL container at 400 K. What is the pressure in atmospheres exerted by this gas? Before you can put the numbers into an equation and solve for the

  11. Chemistry

    How many atoms are there in 6.90 moles of sulfur (S)? Calculate the molar mass of a compound if 0.411 mole of it has a mass of 185 g. Know of any good sites that help answer these ? Or information on how to?

  12. Chemistry

    1. How many moles of Al(CN)3 are in 199 g of the compound? 2. 96.0 mol of P4O10 contains how many moles of P? 3. If 4.71 moles of C5H12 reacts with excess O2, how many moles of CO2 will be produced in the following combustion reaction? C5H12+8O2 ->

  13. Chemistry

    A mass of 0.630 g of NaCl is dissolved in 525 g of water. CAlculate the molality. mass of NaCl= 0.630g mass of H20= 525g molar mass of NaCl= 58.44 This is what i did it keeps telling me the answer is wrong. Convert grams to moles of NaCl 0.630 * 1 mol

  14. chemistry

    if one can find the ratio of the number of moles of the elements in a compound to one another, one can find the formula of the compound. in certain compound of copper and oxygen, Cux Oy, we find that a sample weighing 0.5424g contains 0.4831g Cu. a. How

  15. Chemistry

    Help me out because I attempted these and realized I did not solve them in KJ/Moles. How do you figure out change of enthalpy with the units kJ/moles? My two reactions. First balanced: MgO (s) + 2 HCl (aq) --> MgCl2 (aq) + H2O (l) Second balanced: Mg (s) +

  16. Grade 12 chemistry

    This is the second reaction: HCl(aq)+NaOH(aq)-->NaCl(aq)+H2O(l) (Heat of neutralization) This reaction involves mixing two solutions: 1.00 mol/L NaOH and 1.00 mol/L HCl. Trial 1: 48.0 mL of the NaOH solution is mixed with 47.5 mL of the HCl. The

  17. CHemistry....Please help

    1.SOLUBILITY: At 25C, the molar solubility of calcium phosphate in water is 1.1*10^{-7}M. Calculate the solubility in grams per liter. I m not sure how to convert M to g/L MOLAR MASS OF COLLIGATIVE PROPERTIES: 2.tert-Butyl alcohol is a solvent with a Kf of

  18. Chemistry

    what is the molecular formula of a compound that is 54.5% C, 9.09% H, and 36.4% O. with a molecular weight of 176g/mol. A)C8H16O4 B)C4H8O2 C)C7H12O5 D)C9H18O3 Assume you have 100 g of the substance, then you have 54.5g of C, etc. Moles C= 54.5/12=4.54 mol

  19. Chemistry Dr. Bob

    Now, I'm going to post how to figure out the theoretical yield of carbon dioxide from 1.00g sodium bicarbonate... The reaction of citric acid and sodium bicarbonate is written as H3C6H5O7(aq) + 3 NaHCO3(aq) → Na3C6H5O7(aq) + 3 H2O(l) + 3 CO2(g) Um.. I

  20. chemistry 11

    Hi, I am stuck on a couple questions in chemistry 11. The questions are 1. Calculate the number of moles of the anhydrous salt left behind 2. Calculate the number of moles of water removed by heat from your sample of hydrate. 3. Calculate the moles of

  21. chemistry

    Record and calculate the following masses: (a)mass of empty beaker: 47.420g (b)mass of beaker plus Na₂CO₃:47.920g (c)Mass of Na₂CO₃:0.5g (d)mass of beaker plus NaCl:47.438g (e) Mass of NaCl (g):0.018g **I need help with these questions below** 2.

  22. Chemistry

    Balance Eq.: Na2Co3+ CaCl2--> CaCo3+ 2NaCl. (CHALK) Calculate the mass of a dry precipitate. Calculate the mass of moles of the precipitate produced in the reaction.

  23. Chemistry

    We will calculate the amount of acid to use in each titration. Assume that you are using 0.0512 M NaOH(aq). A good volume of NaOH(aq) to use per titration is 15 mL. From this molarity and volume, the moles of NaOH can be calculated. Since the unknown acid

  24. GK..please check...Chemistry Help Please

    Moles of S203^2- = (molarity)(volume): =(0.032400 mol/L)(0.053 litres S203^2-) = 0.03240 moles S203^2- Moles if I2 based on Equation #2: Moles I2 = (1/2)( 0.03240 moles S203^2-) = .00086 moles I2 Moles of ClO^- based on Equation #1: Moles ClO-(aq) =

  25. Chemistry

    My Question is: Commercial vinegar usually has a concentration of 5%, per volume. Calculate the [H3O+], if the density of acetic acid is 1.051 g/mL. What I did was: mass = V * density mass = 0.05 * 1.051 = 0.05 g moles = grams/molar mass = 0.05/60.05 = 8.3

  26. Chemistry

    A 43.0 g sample of hydrated cobalt (II) sulfite is heated to drive off the water. The anhydrous cobalt (II) sulfite has a mass of 26.1 g. Calculate the mass of water. Calculate the moles of water. Calculate the moles of cobalt (II) sulfite. Calculate the

  27. Chemistry

    I was doing a lab experiment on the reaction of copper(II) sulphate and aluminum: 1) I measured 2.02g of copper(II) sulphate pentahydrate 2) I dissolved the copper(II) sulphate pentahydrate in 10mL of distilled water 3) I added 2.0mL of concentrated HCl to

  28. chemistry

    2C2H6(g)+7O2(g)--> 4Co2 (g)+6H2O(l) A) if 3.00 moles of C2H6 and 9.00 moles of O2 are introducedinto an empty container at 32.0 degree C and then ignited tointiate the above reaction calculate the mass of water that isproduced. B) if the container volume

  29. chemistry

    how many grams of sodium carbonate are needed to prepare 0.250 L of an 0.100 M aqueous solution of sodium ions? well normally you go moles=grams/molar mass than M= moles/L but when looking for grams? what do you do........multiple .250 by .100 than divide

  30. college physics HELP

    A vertically oriented spring stretches 0.2m when a 0.4kg mass is suspended from it. The mass is pulled, stretching the spring by an additional 0.15m. The mass is released and beings to oscillate in SHM. a)Calculate the spring constant for the spring.

  31. "Given Molality, calculate..."

    "Given: An aqueous solution of C6H12O6 with a density of 1.18 g/ml" I) Calculate Molarity 1) It firsts asks me to, "State the moles of solute" 2) Calculate the mass of the solute in grams - I think I can do this if I know how to get #1 3) Later it also

  32. Chemistry

    Mass (before reaction): test tube + HCl(aq) + stir bar + capsule 26.600 g Mass (after reaction): test tube + HCl(aq) + stir bar + capsule 25.300 g Volume of water displaced from the squirt bottle 148 mL Temperature of the CO2(g) 287.4 K Pressure (atm)

  33. Stiochiometry

    Equation 2Mg+O2= 2MgO Lab data: Magnesium ribbon= .04 grams Magnesium Oxide= .09 2. Using the initial mass of magnesium, calculate the moles of oxygen and then moles of magnesium oxide produced. What is the mole ratio of the reactants? 3. Calculate the

  34. chimestry

    more volume of NaOH means more moles of NaOH (volume * molarity = mole ; molarity=constant) , more moles of NaOH means more grams and mole of HCl and more grams and/or mole and/mass of M2CO3 (note that they are both on the same side of the reaction) now

  35. chem

    assuming you have o.4g of Y(OH)3, calculate the mass of BaO2 required to react stoichiometrically to produce YBa2Cu3O7. Now calculate the mass of CuO. Please HELP! Write the balanced equation. Then, calculate the moles of Y hydroxide from .4 g. Then,

  36. chem

    mass of mg- .28 mass of o- .41 calculate the moles of mg and o what is the simples whole number ratio of the moles of mg to the moles of o? round off to the nearest whole number ratio. use this mole ratio to write the empirical formula. the molecular mass

  37. chemistry/ molarity, molality

    A solution is made by mixing 20.0 mL of C6H5CH3, d=.867g/mL, with 140.0mL of C6H6, d=.874g/mL. assuming that the volumes add upon mixing, what is the molarity? what is the molality? i know that molarity= moles/L and molality= moles sol/kg solvent... but im

  38. Chemistry

    SrH2 +2H2O = Sr(OH)2 + 2H2 You wish to calculate the mass of hydrogen gas that can be prepared from 7.74g of SrH2 and 6.45g of H2O How many moles of H2 can be produced from the given mass of SrH2? How many moles of H2 can be produced from the given mass of

  39. chemistry

    2C2H6(g)+7O2(g)--> 4Co2 (g)+6H2O(l) A) if 3.00 moles of C2H6 and 9.00 moles of O2 are introducedinto an empty container at 32.0 degree C and then ignited tointiate the above reaction calculate the mass of water that isproduced. B) if the container volume

  40. Chemistry :/

    Experiment 1 results: mass of crucible 88g mass of hydrate 93g mass of salt 91.196g 1. Calculate the following: a:mass of water in the hydrate sample (g) b:number of moles of water in the sample c:mass of pure salt in the sample (g) d:number of moles of

  41. chemistry

    find the mass of silver chloride formed from 33.2ml of a 0.100M solution of silver nitrate and 200ml of 0.200M solution of calcium chloride solution Solution plan:use mass to mass calculations mass of AgNO3-moles of AgNO3-moles of AgCl-mass of AgCl

  42. Chemistry

    Suppose a student diluted and titrated a bleach unknown exactly as described in the experimental procedure, except only a single titration was performed which required 13.73 mL of 0.100 M Na2S2O3. The density of the original, undiluted bleach unknown was

  43. Chemistry

    1. How many moles of Al(CN)3 are in 199 g of the compound? 2. 96.0 mol of P4O10 contains how many moles of P? 3. If 4.71 moles of C5H12 reacts with excess O2, how many moles of CO2 will be produced in the following combustion reaction? C5H12+8O2 ->

  44. chemistry needs another look plz

    Posted by Lori on Tuesday, December 14, 2010 at 5:38pm. The mole fraction of an aqueous solution of potassium perchlorate is 0.125. Assuming that the density of this solution is 1.20g mL-1, calculate the following: (A) the mass percent of potassium

  45. Chem

    A -> 3C The molar mass of A is 10.0g/mol If 2.0 grams of A reacts, how many moles of C will be produced? A -------------------> 3C m.mass= 10.0g/mol mass = 2.0 g moles = 2.0 g/10.0 g/mol =0.2 mol moles of c = 3 x 0.2 = 0.6 mol Did I do this correctly?

  46. Chemistry 11

    So I did a lab determining the chemical formula of a hydrate. We had to find the molecular formula of a hydrate of copper (2) sulphate, CuSO4 .xH2O. My observation table looks like this: Mass of clean, dry test tube: 21.6g Mass of test tube + hydrated

  47. CHEM

    Air is approximately 80% nitrogen and 20% oxygen (on a mole basis). If 6 g of hydrogen is added to a 22.4 liter maintained at 0 degrees c and initially filled with air at 1 atm pressure, what will be the molecular mass (i.e. the average molecular mass) of

  48. Chemistry help emergency? (theoretical mass/mol)

    I am supposed to calculate the theoretical mass and moles of Cu. However I am given the mass of 2 reactants in the balanced equation: 3CuCl2*2H2O + 2Al -> 3Cu + 2AlCl3 + 6H2O I am given the mass of CuCl2*2H2O to be 0.477g and the mass of Al is 0.267g. If I

  49. Chemistry

    In this lab experiment you will make 100.0 mL of a 0.100 M solution of Co(NO3)2. However you must calculate the number of moles of compound that will be needed (moles= Molarity x Liters).Then calculate the mass of Co(NO3)2 that will need to be weighed out

  50. college general chemistry

    calculate the lowest whole number ratio of Moles of Mg/moles of O average of Moles of Mg/Moles of O Trial 1 mass of empty crucible and lid= 36.560 mass of Mg=0.348 mass of crucible, lid, and product=38.229 Trail 2 mass of empty crucible and lid=32.221 mass

  51. Chemistry

    What mass of solid potassium sulfate, K2SO4, is used to make up exactly 100.0cm^3 of 0.100 mol/dm^3 SO4^2-? This should be a very easy, 1-mark question but for some reason I can't wrap my head around it. moles = mass/Mr, so all you gotta do is moles x

  52. chemistry - synthesis of aspirin

    This is an experiment for a synthesis of aspirin lab mass of salicylic acid = 2.005 g mass of acetic acid = ? moles of acetic acid = ? volume of acetic anhydride = 4 ml mass of acetic anhydride (Use 1.08 g/ml for the liquid density) = (1.08 g/ml) (4 ml) =

  53. Chemistry help

    I am confused as to how to solve the below problem. I am not sure which formula to use. At first I thought I calculate the molar mass of NaOH, followed by calculating moles of NaOH. But I don't have the mass of NaOH to calculate moles. Do I convert 10mL to

  54. chemistry

    A sample of solid monoprotic acid with molar mass equal to 169.7 g/mol was titrated with 0.1599 M sodium hydroxide solution. Calculate the mass in grams of acid to be used if the volume of NaOH to be used is 25 mL. Is the solution correct?: moles NaOH =

  55. college general chemistry

    calculate the lowest whole number ratio of Moles of Mg/moles of O mass of empty crucible and lid= 36.560 mass of Mg=0.348 mass of crucible, lid, and product=38.229

  56. chemistry

    A lighter contains 3.59 g of butane. How many moles of butane are present at STP? Thoughts: So, correct me if I'm wrong however is it appropriate just to calculate its molar mass, and then use that molar mass and the given mass to figure out moles??

  57. chemistry

    I need help with Part 2 Part 1. Record the following for each of the three experiments: (a) Mass of the empty calorimeter (g): 11.600 g (b) Initial temperature in the calorimeter (C): 21.00 (c) Maximum temperature in the calorimeter from the reaction (C):

  58. chemistry

    vinegar/water = 0ml/35ml initial mass (g) = 82.420 final mass with AS(g) = 84.925 How do I figure out initial mass of AS (g)= mass of CO2 evolved = moles of CO2(moles)= Mass of NaHCO3 (g)=

  59. stoichiometrics

    What is the mass of each and which is greater? 1g H2 + ?N2 and 1g H2 + ?O2 I've balanced them to this point: 3H2 + N2 ===> 2NH3 2H2 + O2 ===> 2H2O Help please, I am stuck on this step and cannot get any further. Thanks, PJ Good! You've done the hard part.

  60. chemistry

    Hey, I need help finding out how many moles of CO2 is produced from this reaction. Any help is appreciated, thanks. Mass of empty Erlenmeyer flask (g): 88.000 g Mass of Erlenmeyer flask and 20 mL H2SO4: 112.198 g Mass of 20 mL H2SO4: 24.198 g Trial I Mass

  61. chem

    Assuming that you have 0.4g of Y(OH)3, calculate the mass of of BaO2 required to react stoichiometrically (1Y:2Ba:3Cu) to produce YBa2Cu3O7. Now calculate the mass of of CuO required to react stoichiometrically (1Y:2Ba:3Cu) to produce YBa2Cu3O7. please

  62. Chemistry

    I was doing a lab experiment: 1) I measured 2.02g of copper(II) sulphate pentahydrate 2) I dissolved the copper(II) sulphate pentahydrate in 10mL of distilled water 3) I added 2.0mL of concentrated HCl to the solution and mixed well 4) I added 0.25g on

  63. Chemistry Conversions

    Convert to Mass Convert to Mass: .000523 moles of C6H12O6 if figure that out, would i have to add up the molar mass of C x 6, H x 12 and O x 6 ? then us the total mass of that over moles to find out?

  64. Chemistry

    Many metals react with oxygen gas to form the metal oxide. For example calcium reacts: 2Ca(s) + O2(g)--> 2CaO(s) Calculate the mass of calcium prepared from 4,20g of Ca and 2.80g of O2. (a) How many moles of CaO can form from the given mass of Ca? (b) How

  65. chemistry help!!

    How do I calculate the average Z molar mass, 1/n (Summation) of n*M given this data: (Ave molar mass, mass of sample): (7.5,9.6) , (12.5,8.7), (17.5, 8.9), (22.5, 5.6), (27.5, 3.1), (32.5,1.7) mili moles for repective numbers: 1.3,.7,.51,.25,.11,.052

  66. chemistry - synthesis of aspirin

    I wanted to calculate the theoretical and actual yield of aspirin. mass of salicylic acid = 2.005 g But isn't salicylic acid differ. from acetic acid? If so, how do we find the mass of acetic acid in this experiment volume of acetic anhydride = 4 ml mass

  67. College Chemistry

    We will calculate the amount of acid to use in each titration. Assume that you are using 0.0512 M NaOH(aq). A good volume of NaOH(aq) to use per titration is 15mL. From this molarity and volume, the moles of NaOH can be calculated. Since the unknown acid

  68. Chemistry

    Hi I need help with these following questions. I have all of the data needed. Calculate the enthalpy change of the reaction for each trial (in kJ) 3. Calculate the heat released by the reaction for each trial (in J): 2. Calculate the heat absorbed by the

  69. Chemistry

    Since the unkown acid is monoprotic, this also equals the number of moles of acid to use. A typical molar mass for an unknown acid in this experiment is 380 g/mol. Using this molar mass, calculate the mass (in grams) of unknown acid you should use per

  70. Determination of ASA Content of Tablets Lab Report

    Not asking for answers necesarily but I would to know how to approach each question Mass of pure acetylsalicylic acid (ASA) : .508 g Dilution Absorbance (a.u.) 2:11 .116 4:11 .259 6:11 .392 8:11 .502 10:11 .548 Mass of tablet : .380 g Absorbance read on

  71. CHEM

    A gaseous hydrocarbon (an organic compound consisting of C & H) weighing 0.232g occupies a volume of 102mL at 23 degrees Celcius and 749mmHg. Calculate the molar mass and identify the compound. The compound is: a)C2H4 b)C3H6 c)C4H8 d)C5H10 e)C6H12 How is

  72. Chemistry- Reacting Masses Calculations

    Hi the question asks me to calculate the mass of calcium carbonate that must be decomposed to produce 14kg of calcium oxide. I think I've gone wrong somewhere, do you write 14000g or 14kg etc, could you help? I did: Moles CaO=(Mass CaO/Mr CaO) =1400/56 =25

  73. Chemistry

    I am working on a redox stoichiometry lab. I need to calculate the moles NaBO3*4H2O. Mass=1.0133g in 100mL solution In my experiment I used 9.98mL and titrated in with KMnO4. I'm really confused about how to calculate the moles. Thanks for any help!!!!

  74. Chemistry

    Experiment 1 results: mass of crucible 88g mass of hydrate 93g mass of salt 91.196g 1. Calculate the following: a:mass of water in the hydrate sample (g) b:number of moles of water in the sample c:mass of pure salt in the sample (g) d:number of moles of

  75. science chemistory

    CaCO3 2HCl forms CO2 CaCl2 H2O 1.calculate the molar mass of calcium chloride produce 2.calculate the number of moles of calcium carbonate 3.calculate the mass of calcium carbonate

  76. chem

    Will someone help me with this problem, please? Calculate the mass in grams of 1.20*10^24 molecules of CO2. Well, convert it to moles of CO2. number moles= 1.2*1024/avagnumber Now, you take the molecular mass of CO2 (12 + 2*16) and multiply that by the

  77. Chem

    We will calculate the amount of acid to use in each titration. Assume that you are using 0.0512 M NaOH(aq). A good volume of NaOH(aq) to use per titration is 15 mL. From this molarity and volume, the moles of NaOH can be calculated. Since the unknown acid

  78. Chemistry

    Assume that lemon Juice os 0.05M, the mass of the 5.0ml should be about 5 grams. So the Mass of acid in your sample is about 0.25 grams. Using this and the moles of acid calculate the gfm of the acid in the lemon juice. I was able to calculate moles, but

  79. chemistry

    Use the molar mass of the following in order to calculate the number of moles from the given masses. Watch the significant figures a) 0.025 g of oxygen b)0.657 g og copper c) 0.7 g of chlorine I know how to calculate with finding the molar mass but not

  80. Chemistry

    I have realized I don't understand Avagado's number at all My book shows me this diagram instead of just providing a simple formulas that makes no sense at all here is what I have made sense of so far (6.022 x 10^23 atoms/mol)(mass of element) = molecular

  81. CHEM HELP

    I asked this already but for some reason the answer I got isnt being accepted online Question: In the laboratory, 3.50 grams of salicylic acid were reacted with 7.20 ml of acetic anhydride (density equal to 1.08 g/ml). Determine the limiting reagent. I

  82. sci/chemistry

    when 1.87 g of gypsum(hydrated calcium sulfate) was heated to constant mass, it lost 0.39 g of water. What is the formula of gypsum? YOu know it is of the form: CaSO4.XH2O the idea here is to find x. calculate the number of moles of water in .39g.

  83. chemistry

    formula: 2KClO3 + NaCL = 2KCl + NaCl + 3O2 MASS OF TEST TUBE & MIXTURE = 34.03 G MASS OF EMPTY TEST TUBE = 31.29 G MASS OF MIXTURE = 2.74 G 1ST WEIGHT OF TEST TUBE & RESIDUE =33.64 G FINAL WEIGTH OF TEST TUBE & RESIDUE = 33.64 G MASS OF RESIDUE = 2.35 G

  84. chemistry - DrBob222

    For this question can u please explain steps 3 and 4 4.0 g of ferrous ammonium sulphate, FeS04(NH4)2 SO4 6H20, is used. The oxalate is in excess, calculate the theoretical yield of the iron complex. Can someone please show me how to calculate a question

  85. chemistry

    calculate the molar mass of an unknown whose mass was 0.846 g, and occupied a volume of 354 cm3 at a pressure of 752 torr and a temperature of 100 degrees celcius. I came up with .0114 moles, I want to know if this is correct.

  86. chemistry

    I need help with this lab. Write the equation for the decomposition of the hydrate, CuSO4*XH2O. Mass of crucible and hydrate: 93.000g Mass of crucible and pure salt: 91.196g I need to calculate the following: 1. mass of water in hydrate sample(g) 2. number

  87. chemistry

    I need some help with calculating percent yield and percent purity of aspirin. Here's my data (questions follow): SYNTHESIS Mass of salicylic acid.., 2.0 g Volume of acetic anhydride.., 5 mL Mass of watch glass.., 22.10 g Mass of aspirin and watch glass..,

  88. chemistry

    you wish to calculate the mass of hydrogen gas that can be prepared from 4.89 g of SrH2 and 5.28 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH2?

  89. chemistry

    How do I calculate the average Z molar mass, 1/n (Summation) of n*M given this data: (alternate equation: MZ=Summation N*M^3/Summation N*M^2) (Ave molar mass, mass of sample): (7.5,9.6) , (12.5,8.7), (17.5, 8.9), (22.5, 5.6), (27.5, 3.1), (32.5,1.7) mili

  90. Chemistry

    I need help with this lab. Write the equation for the decomposition of the hydrate, CuSO4*XH2O. Mass of crucible and hydrate: 93.000g Mass of crucible and pure salt: 91.196g I need to calculate the following: 1. mass of water in hydrate sample(g) 2. number

  91. CHEMISTRY

    Someone please tell me if I'm doing this right... It's due tonight!! Dr. Bob222, Yesterday I posted a question and you answered me with how to calculate it.. Can you tell me if I'm doing this correctly?? Please! Consider the following chemical equation:

  92. Chemisty

    Someone please tell me if I'm doing this right... It's due tonight!! Dr. Bob222, Yesterday I posted a question and you answered me with how to calculate it.. Can you tell me if I'm doing this correctly?? Please! Consider the following chemical equation:

  93. Chemistry

    I had to do a lab and had to calculate the molar mass for a substance with this equation MM=Mrt/pv but we had to calculate the mass of the substance and its temperature experimently. My question is why did we have to boil the liquide in a water containing

  94. chemistry higher

    calculate the volume of hydrogen produced when 6g of magnesium is reacted with 100cm of 1 mol l-1 hydrochloric acid no of moles of Mg= mass/gfm = 6/24.3 = 0.247 moles 1/2 mole of Mg= 1/2 mole of H2 = 0.247 moles x 100 = 24.7cm3 ???

  95. AP Chemistry

    My objective is to find the molar mass of a gas. Is this the correct balanced equation for magnesium ribbon reacting with hydrochloric acid to form hydrogen gas? 2Mg (s) + 2HCL (l) ----> H2 (g) + 2MgCl (aq) Also, I'm required to find the mass of the

  96. CHEMISTRY

    Mass (before reaction): test tube + HCl(aq) + stir bar + capsule 26.600 g Mass (after reaction): test tube + HCl(aq) + stir bar + capsule 25.300 g Volume of water displaced from the squirt bottle 148 mL Temperature of the CO2(g) 287.4 K Pressure (atm)

  97. Chemistry=MOLES!

    I'm having trouble converting moles to grams and finding the mass of molecules. Problems I'm stuck on: What is the mass in grams of .99x10^49 Sodium Chloride Molecules? and How many moles of Cu are in 9.61 grams? and How many moles are in 5.94x10^45 Ne

  98. chemistry

    1. Calculate the volume of carbon dioxide at 273 K and 1.01 * 10^5 Pa which would be produced when 1.25g of calcium carbonate reacts completely with HCL. and 2. When 41.18 cm^3 of a solution of silver ions with concentration of .2040 mol dm^-3 is added to

  99. Chemistry

    A .405 g sample of gas contains .0050 moles. What is the molar mass of this gas? Please round your answer to the tenths place. I am confused by this. Molar mass = mass of sample/moles of sample The answer is either: molar mass = .405g/.0050 = 81 g/mol (I

  100. Chemistry ....Please Double check

    If 4.55 g of sodium sulphide and 15.0 g of bismuth nitrate are dissolved in separate beakers of water which are then poured together, what is the maximum mass of bismuth sulphide, an insoluble compound, that could precipitate? What reactant was the

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