1)how many grams of oxygen gas are required for the complete reaction of 22.7 gr

Question

1)how many grams of oxygen gas are required for the complete reaction of 22.7 grams ofcarbon monoxide?
carbon monoxide (g) + oxygen (g) carbon dioxide (g)

2) According to the following reaction, how many grams of waterare needed to form 25.0 grams of oxygen gas?
water (l) hydrogen (g) + oxygen (g)

3) For the following reaction, 26.9 grams of diphosphorus pentoxide are allowed to react with 9.03 grams of water .
diphosphorus pentoxide(s) + water(l)  phosphoric acid(aq)
-What is the maximum mass of phosphoric acid that can be formed?   grams

-What is the FORMULA for the limiting reagent?

-What mass of the excess reagent remains after the reaction is complete?   grams

4) For the following reaction, 11.6 grams of sulfur are allowed to react with 25.1 grams of carbon monoxide .
sulfur(s) + carbon monoxide(g)  sulfur dioxide(g) +carbon(s)
-What is the maximum amount of sulfur dioxide that can be formed?   grams

-What is the FORMULA for the limiting reagent?

-What amount of the excess reagent remains after the reaction is complete?   grams

5) For the following reaction, 3.57 grams of water are mixed with excess magnesium nitride. The reaction yields 4.05 grams ofmagnesium hydroxide.
magnesium nitride (s) + water (l) magnesium hydroxide(aq) + ammonia (aq)

-What is the theoretical yield of magnesium hydroxide ?

grams

-What is the percent yield of magnesium hydroxide ?

  %

6) For the following reaction, 4.35 grams of diphosphorus pentoxide are mixed with excess water . The reaction yields 4.73grams of phosphoric acid .

diphosphorus pentoxide ( s ) + water ( l )  phosphoric acid( aq )

-What is the theoretical yield of phosphoric acid?

  grams

-What is the percent yield for this reaction ?

  %

7) A 0.4370 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated asAgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 1.1582 g.

What is the mass percentage of chlorine in the original compound?

8) A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide to calcium oxide by heating. How many grams ofcalcium oxide should the student obtain if her solution contains44.0 mL of 0.535 M calcium nitrate?

9) A 2.746 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 6.927 grams of CO2 and 1.216 grams of H2O are produced.

In a separate experiment, the molar mass is found to be 122.1g/mol. Determine the empirical formula and the molecular formula of the organic compound.

10) When 3.407 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 10.32 grams of CO2 and 5.282grams of H2O were produced.

In a separate experiment, the molar mass of the compound was found to be 58.12 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

11) You need to make an aqueous solution of 0.139 M potassium nitrate for an experiment in lab, using a 300 mL volumetric flask. How much solid potassium nitrate should you add? (grams)

12) How many milliliters of an aqueous solution of 0.164 Mchromium(II) bromide is needed to obtain 4.28 grams of the salt?

13) In the laboratory you dissolve 13.9 g of potassium nitrate in a volumetric flask and add water to a total volume of 375 mL.

What is the molarity of the solution?   M.

What is the concentration of the potassium cation?   M.

What is the concentration of the nitrate anion?   M.

14) In the laboratory you dissolve 16.4 g of chromium(II) bromidein a volumetric flask and add water to a total volume of 125 mL.

What is the molarity of the solution?   M.

What is the concentration of the chromium(II) cation?  M.

What is the concentration of the bromide anion?   M.

15) In the laboratory you dilute 4.00 mL of a concentrated 3.00 Mhydrobromic acid solution to a total volume of 75.0 mL. What is the concentration of the dilute solution?

16) You wish to make a 0.153 M perchloric acid solution from a stock solution of 12.0 M perchloric acid. How much concentrated acid must you add to obtain a total volume of 150mL of the dilute solution?

17) How many grams of PbBr2 will precipitate when excess FeBr2solution is added to 51.0 mL of 0.516 M Pb(NO3)2 solution?

Pb(NO3)2(aq) + FeBr2(aq) PbBr2(s) + Fe(NO3)2(aq)

18) How many mL of 0.791 M HI are needed to dissolve 7.30 g ofBaCO3?

2HI(aq) + BaCO3(s) BaI2(aq) + H2O(l) + CO2(g)

19) What volume of a 0.132 M barium hydroxide solution is required to neutralize 13.7 mL of a 0.151 M hydrobromic acidsolution?

20) What volume of a 0.238 M perchloric acid solution is required to neutralize 23.5 mL of a 0.198 M calcium hydroxide solution?

21) An aqueous solution of hydrobromic acid is standardized by titration with a 0.132 M solution of barium hydroxide.

If 13.7 mL of base are required to neutralize 13.4 mL of the acid, what is the molarity of the hydrobromic acid solution?

22) An aqueous solution of calcium hydroxide is standardized by titration with a 0.198 M solution of perchloric acid.

If 23.5 mL of base are required to neutralize 19.2 mL of the acid, what is the molarity of the calcium hydroxide solution?

23) A 14.9 g sample of an aqueous solution of hydrobromic acidcontains an unknown amount of the acid.
If 16.5 mL of 0.868 M sodium hydroxide are required to neutralize the hydrobromic acid, what is the percent by mass ofhydrobromic acid in the mixture?

24) A 14.0 g sample of an aqueous solution of perchloric acidcontains an unknown amount of the acid.
If 29.6 mL of 0.192 M sodium hydroxide are required to neutralize the perchloric acid, what is the percent by mass ofperchloric acid in the mixture?

25) For the following reaction, 0.172 moles of magnesium nitride are mixed with 0.365 moles of water.

magnesium nitride (s) + water (l) magnesium hydroxide(aq) + ammonia (aq)

What is the FORMULA for the limiting reagent?

What is the maximum amount of magnesium hydroxide that can be produced?   moles

26) For the following reaction, 0.268 moles of diphosphorus pentoxide are mixed with 0.163 moles of water.

diphosphorus pentoxide (s) + water (l) phosphoric acid(aq)

What is the FORMULA for the limiting reagent?

What is the maximum amount of phosphoric acid that can be formed?   moles

-What is the FORMULA for the limiting reagent?

Explanation / Answer

1)

2CO + O2 ----> 2CO2

2 mol CO = 1 mol O2

No of mol of CO = 22.7/28 = 0.81 mol

No of mol of o2 required = 0.81*2 = 1.62 mol

2)

2H2O ----> 2H2 + O2

nO OF mol of o2 = 25/32 = 0.78 mol

no of mol of water required = 0.78/2 = 0.39 mol

3) diphosphorus pentoxide(s) + water(l) ---> phosphoric acid(aq)

p2o5 + 3H2O ---> 2H3PO4

No of mol of diphosphorus pentoxide = 26.9/283.89 = 0.0947 mol

no of mol of water = 9.03/18 = 0.5 mol

limiting reagent = P2O5

mass of H3PO4 formed = 0.0947*2 = 0.19 grams

mass of excess reagent lleft = (0.5-0.0947*3)*18 = 3.9 grams

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