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19 Nov 2019

Part B-problem solving (please practice the following questions) 1. Predict the products resulting from these aqueous reactions (include phase labels). Write the balanced molecular and net ionic equation. a) AgNO3 + NaI b) Na2CO3 + HCl

6. In the following reaction, 35.6 gram of Al was given to react with 39.4 gram of O2. 4Al(s) + 3O2(g)  2Al2O3(s) (a) Find the limiting reactant. Explain. (b) How many moles of Al2O3 will be produced? (c) How many grams of Al2O3 will be produced?

8. 1.28 g of a compound containing carbon, hydrogen and oxygen (CXHYOZ) is subjected to combustion analysis. The results show that 1.76 g of CO2 and 1.44 g of H2O were produced. Determine the empirical formula of the compound.

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Keith LeannonLv2
13 Apr 2019

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Related questions

#1. Once made by heating wood in the absence of air, methanol (CH3OH) is now made by reacting carbon monoxide and hydrogen at high pressure: CO(g)+2H2(g)→CH3OH(l)

A. If 25.0 g of CO is reacted with 6.00 g of H2, which is the limiting reagent?

B. How many grams of CH3OH can be made from 14.78 g of CO and 5.321 of H2?

#2. For the reaction 4Al(s)+3O2(g)→2Al2O3(s), What is the mass of Al2O3 that is produced when 24.25 g of Al and 24.25 g of O2 react

#3. For the reaction 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g),

What is the mass of HNO3 that is produced when 28.05 g of NO2 and 28.05 g of H2O react?

#4. For each of the following precipitation reactions, calculate how many grams of the first reactant are necessary to completely react with 56.1 g of the second reactant.

A. 2KI(aq)+Pb(NO3)2(aq)→PbI2(s)+2KNO3(aq)

B. 3 Na2CO3(aq)+2FeCl3(aq)→Fe2(CO3)3(s)+6NaCl(aq)

C. K2SO4(aq)+Sr(NO3)2(aq)→SrSO4(s)+2KNO3(aq)

CHM111

Q1. Which of the following contains the MOST atoms? You shouldn't need to do a calculation here.

A) 10.0 g Ne

B) 10.0 g He

C) 10.0 g Ar

D) 10.0 g Kr

E) 10.0 g Mg

Q2. How many atoms are present in 0.23 moles of Calcium?

Q3. How many atoms are present in 5.6 mg of Silicon?

Q4. How many grams of iodine do 5.6 x 1025 atoms of iodine represent?

Q5. Balance the following Chemical Equations:

_____ CaC2(s) + _____H2O(l) ? _____ Ca(OH)2(aq) + _____ C2H2(g)

_____ P4O10 + _____ H2O? ______ H3PO4

___ C3H8O3 + ___ O2 ? ___ CO2 + ___ H2O

_____ C4H10(l) + _____ O2(g) ? _____ CO2(g) + _____ H2O(g)

___ Al + ___ N2 ? ___ Al2N3

___ NaN3 ? ___ Na + ___ N2

___ C3H5N3O9 ? ___ CO2 + ___ N2 + ___ H2O + ___ O2

Q6. Calculate the percent composition of each element in Al(NO3)3

Q7. A 65.0 g sample of a pure compound containing only Nickel, Oxygen and Carbon is found to contain 22.36 g Nickel and 18.27 g Carbon. What is the empirical formula of compound?

Q8. Determine the Empirical formula and Molecular formula of a compound that contains: 65.4% C, 9.15% H and 25.4% N by mass and has a molar mass of 220 g/mol.

Q9. Oxygen gas can be produced by the decomposition of KClO3

2KClO3 (s) ? 2 KCl + 3 O2 (g)

How many grams of O2 can be produced from 1.625 g of KClO3?

Q10. Consider the following balanced reaction: 2 Fe (s) + Al2O3 (s) ® 2 Al (s) + Fe2O3 (s)

If 6.25 moles of Fe react with 2.50 moles of Al2O3

Which reactant is the limiting reagent?

How many grams of Al are produced?

Q11. Consider the reaction for the manufacture of Aluminum sulfate:

2 AlCl3 (aq) + 3 H2SO4 (aq) ? Al2(SO4)3(aq) + 6 HCl (aq)

If 15.0 g of AlCl3was mixed with 25.0 g of H2SO4, which reactant is the limiting reagent?

Calculate the theoretical yield of Al2(SO4)3.

If only 18.63 g of Al2(SO4)3 was produced, what is the percent yield of Al2(SO4)3?

Q13. How many grams of Nickel (II) chloride are needed to prepare 100.0 ml of 0.125 M solution?

Q14. What volume of 0.125 M KMnO4 (aq) solution can be prepared from 12.623 g of KMnO4?

Do Question Number 6

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