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13 Dec 2019

2 Al (s) + 6 HCl (aq) ----> 2 AlCl3 (aq) + 3 H2 (g)

•How many molecules of HCl will react with 4 atoms of Al?

•How many atoms of Al are required to make 1 formula unit of AlCl3?

•How many moles of H2 are made from 3 moles of HCl?

•If 4.5 moles of AlCl3 are produced, what mass of H2 is also produced?

•What mass of HCl is required to react with 1.75 mole of Al?

Could you please show us how you did the work too, thank you :)

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Reid Wolff
Reid WolffLv2
17 Dec 2019

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Related questions

You are given the following unbalanced chemical equation.

Al(OH)3(s) + HCl(aq) → AlCl3(aq) + H2O(l)

How many mL of 2.21 M HCl are required to react completely with 43.4 g of Al(OH)3?
_________ mL

Al(s) + HCl(aq) → AlCl3(aq) + H2(g) 2. According to the equation above, how many grams of aluminum are needed to completely react with 2.19 mol of hydrochloric acid? 3. Sulfur dioxide will react with water to form sulfurous acid SO2(g) + H2O(l) → H2SO3(l) What mass of sulfur dioxide is needed to prepare 27.86 g of H2SO3(l)? 4. The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The chemical equation is shown below. P4S3(s) + O2(g) → P4O10(s) + SO2(g) What mass of SO2 is produced from the combustion of 0.401 g P4S3? 5. How many moles of Mg3P2(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P4(s)? Mg(s) + P4(s) → Mg3P2(s) 6. A 5.95-g sample of AgNO3 is reacted with excess BaCl2 according to the equation AgNO3(aq) + BaCl2(aq) → AgCl(s) + Ba(NO3)2(aq) to give 4.48 g of AgCl. What is the percent yield of AgCl? 7. Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. S8(s) + F2(g) → SF6(g) What is the percent yield if 18.3 g SF6 is isolated from the reaction of 10.0 g S8 and 30.0 g F

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?

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