Balance and classify each reactionSolve the stoichiometry problemShow work Acetylene gas, C2H2, burns in oxygen emitting high temperatures used for welding metals. How many grams of CO2 can be produced when 54.6 g of C2H2 are burned?__ C2H2(g) + __ O2(g) → __ H2O(g) + __ CO2(g)2). How many grams of CO can be produced from a mixture of 70.0 g of SiO2 and 50.0 g of C?__ SiO2(s) + __ C(s) → __ SiC(s) + __ CO(g)3) If 3.40 grams of NH3 are mixed with 8.00 grams of F2, how many grams of HF can be produced?__ NH3(g) + __ F2(g) → __ N2F4(g) + __ HF(g)4) Iron (III) oxide reacts with carbon monoxide to give iron metal and carbon dioxide. If you begin the reaction with 24.0 g of iron (III) oxide and 34.0 g of carbon monoxide, what is the theoretical yield in grams of carbon dioxide?__ Fe2O3(s) + __ CO(g) → __ Fe(s) + __ CO2(g)5) Calcium cyanamide (CaCN2) reacts with water to afford calcium carbonate and ammonia according to the reaction below. If 5.56 g of CaCN2 is mixed with 12.2 g of water, what is the theoretical yield of ammonia? Indicate which reactant will have zero grams at the end of the reaction and which one will have more than zero grams.___ CaCN2(s) + ___ H2O(l) → ___ CaCO3(aq) + ___ NH3(aq)6) Copper reacts with nitric acid to afford copper (II) nitrate, nitrogen monoxide and water. If you react 25.0 g of copper with an excess of nitric acid, what is the theoretical yield of nitrogen monoxide? If the reaction produces 7.24 g of nitrogen monoxide, what is the percent yield?3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l) 7) (a) Calculate the mass in grams of aluminum oxide (Al2O3) produced when 10.0 g of aluminum metal and 19.2 g of oxygen (O2) react. Circle the theoretical yield. Identify the limiting and excess reactant. (b) Calculate the mass of O2 remaining at the end of the reaction.(c) Calculate the actual yield if the percent yield is 66.8%.

Hi there! Thank you for the question, but as per our guidelines we can solve only one question at a time. We’ll answer the first question since the exact one wasn’t specified. Please submit a new question specifying the one you would like to answer.To balance, classify and to solve below stoichiometry problem. Q. Acetylene gas, C2H2, burns in oxygen emitting high temperatures used for welding metals. How many grams of CO2 can be produced when 54.6 g of C2H2 are burned? __ C2H2(g) + __ O2(g) → __ H2O(g) + __ CO2(g) Follow below steps to balance the chemical equation. 1. Balance hydrogen atom in such a way that the number of oxygens atom in H2O is even. 2 C2H2(g) + __ O2(g) → 2 H2O(g) + __ CO2(g) 2. Balance number of carbon atoms on both sides 2 C2H2(g) + __ O2(g) → 2 H2O(g) + 4 CO2(g) 3. Now balance number of oxygen atoms on both sides 2 C2H2(g) + 5 O2(g) → 2 H2O(g) + 4 CO2(g) This is the required balanced equationBecause in the given reaction oxygen combines with acetylene to give water and carbon dioxide therefore the given reaction is a combustion reaction. Molar mass of C2H2 = 26.04 g/molMolar mass of CO2 = 44.01 g/mol From the molar mass, 1 mole of C2H2 = 26.04 g and 1 mole of CO2 = 44.01 g. 2 C2H2(g) + 5 O2(g) → 2 H2O(g) + 4 CO2(g) From the reaction stoichiometry, 2 moles of C2H2 produce 4 moles of CO2 In terms of grams, 2×26.04 g of C2H2 produces 4×44.01 g of CO2 Therefore, 54.6 g of C2H2 produces 4⋅44.012⋅26.0454.6=184.56 g of CO2 Answer: Balanced reaction is:2 C2H2(g) + 5 O2(g) → 2 H2O(g) + 4 CO2(g) It is a combustion reaction 184.56 grams of CO2 can be produced when 54.6 g of C2H2 is burned.

Answered: Balance and classify each reaction…

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...

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Balance and classify each reaction
Solve the stoichiometry problem
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Acetylene gas, C₂H₂, burns in oxygen emitting high temperatures used for welding metals. How many grams of CO₂ can be produced when 54.6 g of C₂H₂ are burned?

__ C₂H₂(g) + __ O₂(g) → __ H₂O(g) + __ CO₂(g)

2). How many grams of CO can be produced from a mixture of 70.0 g of SiO₂ and 50.0 g of C?

__ SiO₂(s) + __ C(s) → __ SiC(s) + __ CO(g)

3) If 3.40 grams of NH₃ are mixed with 8.00 grams of F₂, how many grams of HF can be produced?

__ NH₃(g) + __ F₂(g) → __ N₂F₄(g) + __ HF(g)

4) Iron (III) oxide reacts with carbon monoxide to give iron metal and carbon dioxide. If you begin the reaction with 24.0 g of iron (III) oxide and 34.0 g of carbon monoxide, what is the theoretical yield in grams of carbon dioxide?

__ Fe₂O₃(s) + __ CO(g) → __ Fe(s) + __ CO₂(g)

5) Calcium cyanamide (CaCN₂) reacts with water to afford calcium carbonate and ammonia according to the reaction below. If 5.56 g of CaCN₂ is mixed with 12.2 g of water, what is the theoretical yield of ammonia? Indicate which reactant will have zero grams at the end of the reaction and which one will have more than zero grams.

___ CaCN₂(s) + ___ H₂O(l) → ___ CaCO₃(aq) + ___ NH₃(aq)

6) Copper reacts with nitric acid to afford copper (II) nitrate, nitrogen monoxide and water. If you react 25.0 g of copper with an excess of nitric acid, what is the theoretical yield of nitrogen monoxide? If the reaction produces 7.24 g of nitrogen monoxide, what is the percent yield?

3Cu(s) + 8HNO₃(aq) → 3Cu(NO₃)₂(aq) + 2NO(g) + 4H₂O(l)

7) (a) Calculate the mass in grams of aluminum oxide (Al₂O₃) produced when 10.0 g of aluminum metal and 19.2 g of oxygen (O₂) react. Circle the theoretical yield. Identify the limiting and excess reactant. (b) Calculate the mass of O₂ remaining at the end of the reaction.
(c) Calculate the actual yield if the percent yield is 66.8%.

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Balance and classify each reaction Solve the stoichiometry problem Show work Acetylene gas, C2H2, burns in oxygen emitting high temperatures used for welding metals. How many grams of CO2 can be produced when 54.6 g of C2H2 are burned? __ C2H2(g) + __ O2(g) → __ H2O(g) + __ CO2(g)

Balance and classify each reaction Solve the stoichiometry problem Show work Acetylene gas, C2H2, burns in oxygen emitting high temperatures used for welding metals. How many grams of CO2 can be produced when 54.6 g of C2H2 are burned? C2H2(g) + O2(g) → H2O(g) + CO2(g)