For the chemical reaction shown:\[ 2 \, \text{H}_2\text{O}_2 (l) + \text{N}_2\text{H}_4 (l) \longrightarrow 4 \, \text{H}_2\text{O} (g) + \text{N}_2 (g) \]determine how many grams of \(\text{N}_2\) are produced from the reaction of 9.20 g of \(\text{H}_2\text{O}_2\) and 6.28 g of \(\text{N}_2\text{H}_4\).\[\text{N}_2 \text{ produced: } \underline{\hspace{5cm}} \text{ g}\]

Answered: Image /qna-images/answer/9e5f7c81-6697-43aa-a622-ca352ead1052.jpg

For the chemical reaction shown, 2H₂O₂(1) + N₂H₂(1) - 4H₂O(g) + N₂(g) determine how many grams of N₂ are produced from the reaction of 9.20 g of H₂O₂ and 6.28 g of N₂H4. N₂ produced:

For the chemical reaction shown, 2H₂O₂(1) + N₂H₂(1) - 4H₂O(g) + N₂(g) determine how many grams of N₂ are produced from the reaction of 9.20 g of H₂O₂ and 6.28 g of N₂H4. N₂ produced:

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: What is the mass in grams of NO that will be produced from 51.8 g of NO₂ reacted with excess water…

A: For determining the amount of product, the mole ratio of reactants in a balanced reaction must be…

Q: What is the mass in grams of H2 that can be formed from 54.6 G of NH3 in the following reaction? 2…

A: From the stoichiometry, we can easily calculate , the problem.

Q: 2. Which one of the following compounds is optically inactive? A B E

Q: Starting with the following equation, Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s) calculate the moles of…

Q: How many moles of NH₃ can be produced from 4.93 moles of nitrogen in the following reaction: N₂ (g)…

A: Recall the given reaction N2g + 3 H2g → 2 NH3g Given moles of N2(g) is 4.93 moles

Q: For the chemical equation given below (not balanced), the percent yield of the reaction is 65.0%.…

A: The reaction given is : MgO(s) + Fe(s) → Fe2O3(s) + Mg(s) 3MgO(s) + 2Fe(s) → Fe2O3(s)…

Q: hen 8.00 g of Aluminum is allowed to react with 35.0 g of chlorine gas to produce aluminum chloride,…

A: The limiting reagent in a chemical reaction is a reactant that is totally consumed when the chemical…

Q: Propane (C3H8) burns in oxygen to produce carbon dioxide and water. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)…

Q: Using the following equation, determine the % yield from the following reaction if 3.040E+1 g of…

A: Mass of octane = 30.04 g Mass of CO2 = 81.85 g

Q: If 5.09 mol of C5H12 reacts with excess O2, how many moles of CO2 will be produced by the following…

A: The given reaction is

Q: What mass in grams of magnesium oxide is produced from 2.00 mol of magnesium? What mass of glucose…

Q: An important intermediate reaction in the industrial production process of nitric acid is shown What…

A: Molar mass of NH3 =(14+3×1) g/mol =17 g/molMolar mass of H2O =(2×1+16) g/mol =18g/molMss given of…

Q: TiCl4 (189.68 g/mol), a source of Ti metal, can be produced from titanium dioxide, carbon and…

Q: starting with the equation, KOH(s)+CO2(g)=K2CO3(S)+H2O(L) Calculate the mas in grams of KOH that…

A: Given, KOH(s) + CO2(g) ➝ K2CO3(s) + H2O(l) mass of K2CO3 produced = 285 g mass of KOH required = ?…

Q: Use the balanced equation, 4K + O₂ 2 K₂O, to answer the following question. How many grams of K are…

A: mass of O2 = 19.1 gmolar mass of O2 = 32.00 g/molAtomic mass of K = 39.10 g/mol

Q: How many moles of phosphorus are required to produce 15.5g P4O6 in the following equation? 4 P(s)+ 3…

A: First of all, write the balanced chemical equation for the formation of P4O6. 4 P(s)+ 3 O2(g) →…

Q: Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of…

Q: How many grams of NO will be produced from 80.0 g of NO₂ reacted with excess water in the following…

A: Given, mass of NO2 = 80.0 g Molar mass of NO2 = 46.0 g/mol Molar mass of NO = 30.01 g/mol

Q: For the chemical equation given below (not balanced), the percent yield of the reaction is 65.0%.…

Q: given the following balanced equation 2 Co2O3(s) + 3 C(s) --> 4 Co(s) + 3 CO2(g) indicate the…

A: Given : 2 Co2O3(s) + 3 C(s) --> 4 Co(s) + 3 CO2(g) To determine : subscript on the oxygen in…

Q: Under certain conditions the formation of ammonia from nitrogen with excess oxygen produces a 38.2%…

A: The given balanced equation is as follows. 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) Molar mass of NH3=17…

Q: How many moles of NH3 can be produced from 3.17 moles of nitrogen in the following reaction: N2 (g)…

A: We use the concept of molarity, in the given question. In the given reaction, 1 mole of N2 gives 2…

Q: What is the mass in grams of magnesium chloride that can be produced from 6.68 moles of chlorine gas…

A: Given, Mg(s)+Cl2(g) ➝ MgCl2 moles of chlorine (Cl2) gas reacts = 6.68 moles Excess reactant ➝…

Q: What is the mass in grams of NO that will be produced from 15.7 g of NO₂ reacted with excess water…

A: To solve this problem we will use the Stoichiometry of given Balanced chemical equation .

Q: Starting with the following equation, Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s) calculate the moles of…

A: We have given that Starting with the following equation, Fe2O3(s) + Al(s) -------> Fe(s) +…

Q: Al4C3 (s) + 12 H2O (l) → 4 Al(OH)3 (s) + 3 CH4 (g) In this reaction, 0.3455 mol of…

Q: Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s) calculate the moles of Fe₂O₃ that will be required to produce…

A: The balanced chemical equation for the reaction between Fe2O3 and Al is: Fe2O3(s) + 2Al(s) → 2Fe(l)…

Q: How many grams of NO are required to produce 145 g of N2 in the following reaction? 4NH3(g) + 6NO(g)…

Q: Given the unbalanced chemical equation, CH3OH(I) + O2(g) → CO2(g) + H20(g), what is the mole ratio…

A: Mole ratio from a given chemical equation is found by balancing the equation. Write a balanced…

Q: Methane (CH4) gas undergoes a combustion reaction as shown below. If 10.0 g of methane reacted and…

A: The percent yield is the percentage ratio of actual yield to theoretical yield. Mathematically, it…

Q: What is the mass in grams of NO that will be produced from 65.8 g of NO₂ reacted with excess water…

A: Given, 65.8 g of NO₂ MW of NO2 = 46.0 g/mol Moles=65.846=1.4304 mol of NO2

Q: for the reaction: 2HNO3 + Mg(OH)2 to form Mg(NO3)2 + 2H2O, how many grams of magnesium nitrate are…

A: The objective of this question is to determine the amount of magnesium nitrate produced from a given…

Q: what is the mass in grams of NO that can be formed from 4.96 moles of NO2 in the reaction below…

A: From the reaction we can say that 3 mole of NO2 gives 1 mole of NO . So 4.96 mole of NO2 gives…

Q: An experiment that led to the formation of the new field of organic chemistry involved the synthesis…

A: Balanced chemical equation: 2 NH3 (g) + CO2 (g) → CN2H4O (s) + H2O (l) Number of moles = Mass/molar…

Q: The steel-making process described in the Transition Metal section of the Elements Handbook shows…

A: When two reactive compounds are mixed, then they react according to the stoichiometry of the…

Q: For the balanced equation below, calculate the percentage yield of hydrogen when 5.63 g of magnesium…

A: Given balanced chemical equation is Mg(s) + 2H2O(l) ----------> Mg(OH)2 (s) + H2(g) Mass of Mg…

Q: Starting with the following equation, Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s) calculate the moles of…

A: Given :- Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s) mass of Fe = 755 g To be calculated :- number of…

Q: The equation for the production of glucose through photosynthesis is: 6 CO₂ + 6 H₂O → C₆H₁₂O₆ + 6 O₂…

A: 1 mol = 6.022 x 1023 molecules/ions/entity Mass of 1 mole = molar mass Amount of product formed can…

Q: How many grams of Fe are produced when 65.0 grams of iron (III) oxide is reacted with 52.3 grams of…

Q: how many moles of H2O will be produced from 2.58 moles of O2 accroding ti the above balanced…

A: The mole to mole ratio is the ratio of the coefficient present in the balanced reaction. Use this…

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

100%

For the chemical reaction shown:

\[ 2 \, \text{H}_2\text{O}_2 (l) + \text{N}_2\text{H}_4 (l) \longrightarrow 4 \, \text{H}_2\text{O} (g) + \text{N}_2 (g) \]

determine how many grams of \(\text{N}_2\) are produced from the reaction of 9.20 g of \(\text{H}_2\text{O}_2\) and 6.28 g of \(\text{N}_2\text{H}_4\).

\[
\text{N}_2 \text{ produced: } \underline{\hspace{5cm}} \text{ g}
\]

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

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

Kaolinite, a clay mineral with the formula Al4Si4O10(OH)8, is produced naturally by the chemical weathering of aluminum silicate minerals like feldspar (granite). Kaolinite is used industrially as filler in slick-paper for magazines and as a raw material for ceramics. How many grams of oxygen are present in 14.79 g of kaolinite?
(ii) Magnesium reacts with oxygen to form magnesium oxide. 2Mg + 0, 2M9O 2.43g of magnesium was burned. Calculate the theoretical yield of magnesium oxide. theoretical yield of magnesium oxide =
What is the mass in grams of carbon dioxide that would be required to react with 53.1 g of LiOH in the following chemical reaction? 2 LiOH(s) + CO₂(g) → Li₂CO₃(s) + H₂O(l)
How many moles of sodium chlorate (NaCIO3) are required to produce 0.235 mol O2? 2 NaCIO3(s) – 2 NaCI(s) + 3 O2(g)
What mass of aluminum oxide can be produced from 100.0 g of aluminum given the reaction: 4Al (s) + 3O2(g) --> 2Al2O3
What is the mass in grams of NO that will be produced from 36.8 g of NO₂ reacted with excess water in the following chemical reaction? 3 NO₂(g) + H₂O(l) → 2 HNO₃(g) + NO(g)
Calculate the mass of iron required to produce 0.332 g of silver metal, given this fully balanced reaction. 3AgNo3 (aq) + Fe (s) = Fe(NO3)3 (aq) + 3Ag (s)
A pile of powdered iron with a mass of 0.6891 grams reacted with excess oxygen. When the experiment was complete, it was determined 0.9730 grams of iron (III) oxide had been produced. What is the percent yield for this experiment? 2 Fe(s) + 1.5 O2(g) ⟶⟶ Fe2O3(s)
22.0 g of CO2 gas and 9.01 g of H2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?
How many grams of carbon dioxide would be required to react with 51.2 g of LiOH in the following chemical reaction? 2 LiOH(s) + CO₂ (g) → Li₂CO₃ (s) + H₂O (l)
When heated, Fe(OH) decomposes into Fe2O3 and water, according to the followingequation:2 Fe(OH)3 (s) > Fe2O3 (s) + 3 H20 (g)If 25.96 g of Fe(OH)3 decomposes, and 11.06 g of Fe2O3g are obtained in the reaction,what is the percent yield of the reaction?
Determine the mass of antimony produced when 0.46 grams of antimony (III) oxide reacts with carbon according to the following balanced equation: Sb2O3 (s) + 3 C (s) -----> 2 Sb (s) + 3 CO (g)