2 AL +6 HC →2 All3 +3 Hq balanced rection 7. a) Use the balanced chemical equation above to determine how many grams of hydrogen gas are produced by the reaction of 1.84 g Al with 75.0 mL of 2.95 M HCI. b) Which is the limiting reactant? c) How much excess reactant is left over? d) If the percent yield is 87.5 %, then how much hydrogen gas is obtained?

2 AL +6 HC →2 All3 +3 Hq balanced rection 7. a) Use the balanced chemical equation above to determine how many grams of hydrogen gas are produced by the reaction of 1.84 g Al with 75.0 mL of 2.95 M HCI. b) Which is the limiting reactant? c) How much excess reactant is left over? d) If the percent yield is 87.5 %, then how much hydrogen gas is obtained?

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

Related questions

Q: Combining 0.278 mol Fe,O, with excess carbon produced 17.8 g Fe. Fe,O, + 3 C → 2 Fe + 3 CO What is…

Q: 5. A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of…

A: Limiting reactant :- A reactant which is present in lesser number of molrs than required as per…

Q: In the reaction of 28 g NO2and 18 g H2O by the chemical equation: NO2 (g) + H2O (1)→HNO; (1) + NO…

Q: Given - 1P4 (s) + 5O2 (g) —> 1 P4O10 (g) a) calculate the mass of P4 (s) required to produce…

A: Consider the reaction equation: 1P4(s) + 5O2(g) —> 1 P4O10(g) Molecules of P4O10 = 3.22×1023…

Q: Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The unbalanced…

A: Given: Mg(s)+O2→MgO(s) Mass of Mg=10.1 gMass of O2=10.5 gMass of MgO=11.9 g To determine: Limiting…

Q: In the reaction of 28 g NO2and 18 g H2O by the chemical equation: NO2 (g) + H2O (1) →HNO; (1) + NO…

A: Use stoichiometric calculation for calculation of moles of nitric acid and limiting reagent.…

Q: Ammonia can be produced by the Haber process: ___ N2(g) + ___ H2(g) → ___ NH3(g) 11. Balance the…

A: Determining the balance equation, limiting reagents and percentage of yield

Q: Consider the balanced reaction given below. How many moles of CO2 would form when 0.628 mol of C4H8…

A: given C4H8 = 0.628 mol from equation 1mol C4H8 = 4mol CO2

Q: A 14.559 g sample of CaCl, was added to 12.328 g of K,CO, and mixed in water. A 3.546 g yield of…

A: Limiting reagent:- It is a reactant which is used up completely during the reaction. No further…

Q: Determine the theoretical yield of water if 2.4g of hydrogen gas reacts with excess oxygen gas…

Q: Consider the reaction. 2 Pb(s) + O,(g) → 2 PbO(s) An excess of oxygen reacts with 451.4 g of lead,…

A: Note : As per our guidelines we are supposed to answer first question please resubmit the other…

Q: ZA + 3B → C 4.0 mol A is mixed with 4.0 mol B and a reaction takes place. Which reactant is…

Q: Combustion of propane, C3H8, serves as an energy source in many rural Indiana homes. The unbalanced…

A: The reaction given is, => C3H8 + O2 → CO2 + H2O Given: Moles of propane combusted = 1.00 mol.

Q: Mass of empty 250 mL beaker 99.104g Mass of Copper (II) Sulfate pentahydrate 2.92g mass of iron…

A: The reactant which is available in a quantity that is less than the amount required for complete…

Q: 15.50 g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.50 g AgCl is produced. What is…

A: The balanced reaction taking place is given as, => NH4Cl + AgNO3 ------> AgCl + NH4NO3 Given…

Q: 4. Hydrogen chloride gas can be prepared by the following reaction: 2NaClu) + H2SO4) 2HClg + NazSO)…

A: The molar mass of H2SO4 is 98.079g/mol The molar mass of NaCl is 58.44g/mol

Q: When the following equation is balanced, how many water molecules are present in the reactants?…

Q: H3PO4 + 3NaOH >>> Na3PO4 + 3H2O If you start the reaction with 100. grams of each reactant, which…

Q: mass

Q: 4. The combustion of ethanol (C₂H5OH) produces carbon dioxide and water. In the reaction, 3.50 g of…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: Combining 0.329 mol Fe2O3 with excess carbon produced 18.9 g Fe Fe2O3+3C⟶2Fe+3CO What is the actual…

A: Given:0.329 mol Fe2O318.9 g FeThe chemical equation involved:Fe2O3+3C⟶2Fe+3CO

Q: Combining 0.213 mol Fe,O, with excess carbon produced 18.4 g Fe. Fe,0, + 3C – 2 Fe + 3 CO What is…

Q: Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the…

A: It is based on the concept of stoichiometry and limiting reagent. Here we are required to find the…

Q: Combining 0.392 mol Fe2O30.392 mol Fe2⁢O3 with excess carbon produced 16.7 g Fe.16.7 g Fe.…

Q: Answer the questions about the balanced reaction 3 A + 2 B → 1 C + 100. cal The molar…

A: Given- A+2B->1C+100 cal Molar mass of A=10 gram Molar mass of B=20 gram Molar mass of C=70…

Q: .A balanced chemical reaction and an incomplete reaction map are hown below. What number is missing…

A: 2NaN3 = 3N2+2Na

Q: 32. For the equation given: 2C₂H4 + 60₂ 4H₂O If 14.0 grams of C₂H4 is reacted and the actual yield…

A: A balanced chemical equation contain equal number of atoms of each elements on both sides of the…

Q: Combining 0.332 mol Fe₂O3 with excess carbon produced 13.0 g Fe. 2 Fe₂O3+3C →2 Fe + 3 CO What is the…

A: The objective of the question is to calculate the actual yield, theoretical yield and percent yield…

Q: Determine the limiting reactant (LR) and the Theoretical Yield (in g) of nitrogen that can be formed…

Q: Combining 0.315 mol Fe,0, with excess carbon produced 18.0 g Fe. Fe,0, + 3C - 2 Fe + 3 CO What is…

Q: e limiting reagent?

Q: → SF6 If you need to make 35 moles of SF6, how many moles of each reactant are required?

A: The given equation is unbalanced. It is needed to be balanced for solving this kind of problem. Each…

Q: How many moles of N2(g) are produced by the decomposition of 390 g NaN3 under the following…

Q: A mixture of 4.5 moles of aluminum and 3.0 moles of oxygen is allowed to react: 4 Al(s) + 3 O₂(g) →…

Q: For the following unbalanced equation, calculate how many grams of each product would be produced by…

A: Well, first of all, we have to balance the reaction. and using the mole ratio one can calculate the…

Q: For the reaction 2KClO3(s)→2KCl(s)+3O2(g) calculate how many grams of oxygen form when each…

A: The balanced reaction given is, => 2 KClO3 (s) ------> 2 KCl (s) + 3 O2 (g) Molar mass of…

Q: Combustion of 8.45 mg of an unknown substance yields 14.0 mg CO2 and 7.08 mg H20. The unknown…

A: We have to calculate the % of each element in substance.

Q: Refer to this equation: 3SCl2 + 4NaF --> SF4 + S2Cl2 + 4NaCl 64.0 grams SCl2 is reacted with…

A: Given chemical equation: 3SCl2 + 4NaF --> SF4 + S2Cl2 + 4NaCl Number of moles =(given…

Q: Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum…

A: The reaction between MnO2 and Al –metal is shown as: Here, MnO2 and Al react in 3:4 ratio. Given…

Q: Combining 0.218 mol Fe, O, with excess carbon produced 10.6 g Fe. Fe,0, +3C- 2 Fe + 3 CO What is the…

A: Given :- Fe2O3 + 3C →2Fe + 3CO Number of moles of Fe2O3 = 0.218 mol Mass of Fe actually produced…

Q: In the reaction of 28 g NO2and 18 g H2O by the chemical equation: NO2 (g) + H2O (1)→HNO; (1) + NO…

A: Given:- Reaction:- NO2 (g) + H2O (l) -> HNO3 (l) + NO (g) 28 g of NO2 used 18 g of H2O used

Q: Combining 0.288 mol Fe,0, with excess carbon produced 16.2 g Fe. Fe,0, +3C – 2 Fe + 3 CO What is the…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

2 AL +6 HC
→2 All3
+3 Hq
balanced rection
7. a) Use the balanced chemical equation above to
determine how many grams of hydrogen gas are produced
by the reaction of 1.84 g Al with 75.0 mL of 2.95 M HCI.
b) Which is the limiting reactant?
c) How much excess reactant is left over?
d) If the percent yield is 87.5 %, then how much hydrogen
gas is obtained?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Determine percent yield for the reaction. Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(�)+O2(�)→2MgO(�) When 10.1 g of Mg are allowed to react with 10.5 g of O2, 11.6 g of MgO are collected.
15.50 g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.50 g AgCl is produced. What is the actual yield of AgCl? NH4Cl + AgNO3 --> AgCl + NH4NO3
10. Balance the equation for the combustion of butane, C,H,. C.H10 + O, > со, + H2O a. If 31.4 grams of butane burn according to this reaction, how many grams of oxygen would you need to ensure all the butane burned? (112 g O,)
Consider the reaction. 2 Рb's) + O,(g) — 2 PЬО(s) An excess of oxygen reacts with 451.4 g of lead, forming 348.1 g of lead(II) oxide. Calculate the percent yield of the reaction. percent yield: % * TOOLS x10
Combining 0.333 mol Fe, O, with excess carbon produced 12.7 g Fe. Fe,0, + 3C → 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: mol What is the theoretical yield of iron in moles? theoretical yield: mol What is the percent yield? percent yield: %
What is the total mass of products formed with 16 grams of methane (CH4) is burned with excess oxygen?
How many grams of H20 will be formed when 31.78 mol H2 is mixed with 2.64 mol of O2 and allowed to react to form water according to the reaction below? 2H2 + 02 2H20 -----> (Note: Determine the limiting reagent first) A 23.6 g B 286 g c) 94.6 g D 47.3 g E 144 g
When 33.9 g of CH4 reacts completely with excess chlorine yielding 52.0 g of HCI, what is the percentage yield, according to CH418) + Cl2g) - CH3Clg) + HClig) 67.2 34.8 65.2 32.8 O 77.3
For the following reaction, 0.497 moles of sulfur are mixed with 0.217 moles of carbon monoxide. What is the formula for the limiting reagent? What is the maximum amount of sulfur dioxide that can be produced? sulfur(s) + carbon monoxide(g) -> sulfur dioxide(g) + carbon(s)
Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is 2Mg(s)+O2(g)→2MgO(s) When 10.0 g Mg is allowed to react with 10.5 g O2, 11.8 gMgO is collected. 1. Determine the theoretical yield for the reaction. 2. Determine the percent yield for the reaction.
given the chemical equation Zn+2HCl->ZnCl2+H2 how many molecules of H2 will be produced if 19 Atoms of ZN are consumed in the reaction
In the reaction of 28 g NO2and 18 g H2O by the chemical equation: NO2 (g) + H2O (1) → HNO3 (1) + NO (g) a- Balanced the reaction equation. b- Calculate the moles of given reactants. c- Calculate the moles of product, HNO3. d- Calculate the mass of HNO; formed in grams. e- Which of the reactants is the limiting reagent? N=14g/ mol, O = 16g/mol,H=1 g/mol. wwm