Question

In: Chemistry

A)An exactly 500 gram iron ore sample was determined to contain 242 grams of iron. What...

A)An exactly 500 gram iron ore sample was determined to contain 242 grams of iron. What is the mass percent of iron in the ore?

B) What are the coeffieceints for the following properly balaned reaction-

__Sodium phosphate reacts with___barium nitrate to from ___sodium nitrate and ____barium phosphate

C) What mass of iron is present in a 6.03 gram sample of iron (II) chloride?

Solutions

Expert Solution

A)    mass percent of iron in the ore = mass of iron/ mass of iron ore x 100

                                                         = 242 grams / 500 grams x 100

                                                          = 48.4 %

B)  2 Na3PO4 + 3Ba(NO3)2 -------------> 6NaNO3 + Ba3(PO4)2

C)

     mass of iron is present in a 6.03 gram sample of iron (II) chloride

         = [molar mass of Fe / molar mass of FeCl2] x mass of sample

         = [55.8 g / 126.7 g ] x 6.03 grams

         = 2.65 grams

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

The mass of a sample or iron ore is known to be 35.714 grams. You measure...
The mass of a sample or iron ore is known to be 35.714 grams. You measure the mass of this sample using three different scales and obtain the following masses: 36.2 g, 35 g, 34.9 g and 35.9 g. The accepted tolerance for both error and for accuracy is 2%. With respect to accuracy and precision, how would you best describe these measurements? Hint: Determine the average mass, absolute deviation for each trail, the M.A.D, and Relative Deviation (percent).
a 35.0 gram sample of ethylene glycol, is dissolved in 500 grams of water The vapor...
a 35.0 gram sample of ethylene glycol, is dissolved in 500 grams of water The vapor pressure of pure water at 32.0 degrees Celsius at 35.7 torr. what is the vapor pressure of the solution at 32.0 degrees Celsius?
What is the percentage of Fe2O3 in a sample of limonite ore if the iron from...
What is the percentage of Fe2O3 in a sample of limonite ore if the iron from a 0.5000-g sample is reduced and titrated with 35.15 ml of a potassium dichromate solution of which 15.00 mL is equivalent in oxidizing power to 25.00 mL of a potassium permanganate solution which has an iron value of 0.004750 g?
The zinc content of a 1.64 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.64 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc, and then neutralizing excess HCl with NaOH. The reaction of HCl with Zn is shown below. The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.71 mL of 0.510 M NaOH for the HCl...
The zinc content of a 1.64 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.64 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc, and then neutralizing excess HCl with NaOH. The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.71 mL of 0.510 M NaOH for the HCl present to be neutralized. What is the mass percentage...
The zinc content of a 1.40 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.40 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc, and then neutralizing excess HCl with NaOH. The reaction of HCl with Zn is shown below. Zn (s) + 2HCl (aq) --> ZnCl2 (aq) + H2 (g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final...
The zinc content of a 1.17 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.17 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc, and then neutralizing excess HCl with NaOH. The reaction of HCl with Zn is shown below. Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.50 mL...
The gravimetric analysis of iron in an ore sample was performed by digesting the sample in...
The gravimetric analysis of iron in an ore sample was performed by digesting the sample in strong acid, followed by precipitation of Fe(OH)3 using KOH, filtration of the crystalline iron hydroxide, and finally drying and ignition at high temperature to produce Fe2O3. After cooling in a dessicator, two different students got the following replicate results: Student 1, Trial 1 – 0.2109 g of ore results in 0.04594 g iron (III) oxide Student 1, Trial 2 – 0.2110 g of ore...
The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl,
The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HCl is then neutralized with with NaOH. The reaction of HCI with Zn is shown. Zn(s)+2 HCl(aq) → ZnCl2 (aq) +H2 (g) The ore was dissolved in 150 mL of 0.600 M HCI, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.22 mL of...
A 20 gram iron block at an initial temperature of 20oC is placed in 20 grams...
A 20 gram iron block at an initial temperature of 20oC is placed in 20 grams of water at an initial temperature of 80oC. Assuming no heat is lost to the surroundings, what would be the final temperature of the system once you reach thermal equilibrium? CSiron=0.449JgoC CSwater=4.18JgoC 74.2o C 80.0o C 25.8o C 50.0o C 112o C
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT