**Text Transcription for Educational Website:**13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (Al₂S₃) according to this balanced chemical equation:\[ 2 \text{Al} (s) + 3 \text{S} (s) \rightarrow \text{Al}_2\text{S}_3 (s) \]**Question:** How many atoms of aluminum will react completely with 1.33 × 10²³ atoms of sulfur?**Explanation:** This is a stoichiometry problem that involves calculating the amount of aluminum atoms needed to react with a given number of sulfur atoms, based on the balanced chemical equation provided. To find the answer, use the stoichiometric ratio from the equation. For every 3 sulfur atoms, 2 aluminum atoms are required to form aluminum sulfide.

We will solve this question using stoichiometric calculations.

13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (ALS) according to this balanced chemical equation: 2 Al(s) +3 S(s) → AlS(s) How many atoms of aluminum will react completely with 1.33 x 104 atoms of sulfur?

13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (ALS) according to this balanced chemical equation: 2 Al(s) +3 S(s) → AlS(s) How many atoms of aluminum will react completely with 1.33 x 104 atoms of sulfur?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the reaction of solid aluminum iodide and potassium metal to form solid potassium iodide and aluminum metal. The balanced chemical equation is AlI₃(s) + 3 K(s) → 3 KI(s) + Al(s). What quantity in moles of aluminum are produced if 1.34 moles of aluminum iodide are reacted with 3.21 moles of potassium based on the balanced chemical equation?
Catalytic converters are the most common option for controlling emissions of polluting gases by internal combustion engines in automobiles, accelerating the conversion of nitrogen oxides into nitrogen and oxygen gases. A chemical reaction that can be used for the conversion of nitric oxide into non-polluting gases is the reaction of this gas with hydrogen, resulting in nitrogen and water gases, as shown in the chemical equation below: 2 NO(g) + 2 H2(g) → N2(g) + H2O(g) The kinetics of this reaction at a temperature of 1250 °C is represented in the following table, which indicates the influence of the concentration of the reactants on the reaction rate, obtained through three experiments conducted under the same conditions EXPERIMENTO [NO] (MOL/L) [H2] (MOL/L) V0 (MOL/Ls) 1 0,20 0,08 0,05 2 0,40 0,08 0,20 3 0,40 0,16 0,40 Determine the rate law for this chemical reaction, the rate constant, and its respective unit. Calculate the rate when the concentration of NO is 0.30…
How many grams of iron, molar mass 55.85 g/mol, will be consumed during the formation of 13.71 grams of Fe2O3? Report your answer with 3 significant figures. Molar mass of Fe2O3 = 159.69 g/mol 4 Fe + 3 O2 → 2 Fe2O3
Consider the reaction of solid aluminum iodide and potassium metal to form solid potassium iodide and aluminum metal. The balanced chemical equation is AlI₃(s) + 3 K(s) → 3 KI(s) + Al(s). How many moles of aluminum are produced if 1.45 moles of aluminum iodide are reacted with 3.49 moles of potassium based on the balanced chemical equation?
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H₂(g) + N₂ (g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted the chemical equation. 1.56 g H₂ is allowed to react with 10.1 g N₂, producing 2.25 g NH3. Part A What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) Value Submit Part B μÃ Submit What is the percent yield for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) μĂ Value Units Units ? wwwww ?
Classify each chemical reaction: reaction 2CH₂ CH₂CO₂H (1) + 70₂(g) → 6CO₂(g) + 6H₂0(g) CH, (CH₂), CH₂ (8) + 80₂(g) → 5CO₂(g) + 6H₂0 (g) Na₂S (aq) + FeCl₂ (aq) → 2NaCl(aq) + FeS (s) Mg1₂ (aq) + Pb (NO₂)₂ (aqg) → Mg(NO3)₂ (aq) + PbI₂ (s) type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition X precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base
Given the equation, Cu + 2AgNO3 → Cu(NO3)2 + 2Ag: What is the mole ratio of Ag and AgNO3? If 6.25 moles of Ag are created, how many moles of copper (Cu) were reacted? If 5.12 mol Cu(NO3)2 were formed, how many moles of silver (Ag) were also created?
For the balanced chemical equation, C6H5OH + 7 O2 à 6 CO2 + 3 H2O, if 234 molecules of CO2 are produced, how many molecules of oxygen were used?
14. When propane (C3H8) undergoes complete combustion in oxygen, it produces carbon dioxide and water, as shown in the reaction equation below: 2 C3H3 (g) + 7 02 (g) → 3 CO2 (g) + 8 H20 (g) If 25.00 g of propane are reacted with 25.00 g of oxygen, calculate how many grams of carbon dioxide gas will be formed.
Consider the following balanced equation: 2 H2 + O2 → 2 H2OWhat mass of water (H2O) will be collected if 20.0 grams of oxygen gas (O2) are consumed? (Mass of H2O = 18.02 g/mol and Mass of O2 = 32.00 g/mol)
The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). What is the mass in grams of phosphorus trichloride that can be formed from 226.0 grams of chlorine gas based on the balanced chemical equation?
According to the following reaction, how many grams of mercury will be formed upon the complete reaction of 31.3 grams of mercury(II) oxide? 2HgO(s) → 2Hg(l) + O₂(g) ||| g mercury