Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen: 3H2(g)+N2(g)2NH3(g) In a particular reaction, 6.0 mol of NH3 were produced. How many moles of H2 and how many moles of N2 were consumed to produce this amount of NH3 ?

Short Answer

Expert verified
9.0 moles of H2 and 3.0 moles of N2 were consumed.

Step by step solution

01

Understand the Reaction

The balanced chemical equation for the formation of ammonia (NH3) from hydrogen (H2) and nitrogen (N2) is given by:3H2(g)+N2(g)2NH3(g)This means 3 moles of H2 react with 1 mole of N2 to produce 2 moles of NH3.
02

Set Up the Mole Ratio

From the balanced equation, the molar ratio between H2 and NH3 is 3:2, and between N2 and NH3 is 1:2.
03

Calculate Moles of H2 Consumed

Since the ratio of H2 to NH3 is 3:2, you can set up the proportion:3molH22molNH3=xmolH26.0molNH3Solving for x, 3/2=x/6.0 gives:x=32×6.0=9.0molH2
04

Calculate Moles of N2 Consumed

Since the ratio of N2 to NH3 is 1:2, you use:1molN22molNH3=ymolN26.0molNH3Solving for y, 1/2=y/6.0 gives:y=12×6.0=3.0molN2

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Mole Ratio
In the study of chemical reactions, understanding the concept of mole ratio is essential. Mole ratio is derived from the coefficients of a balanced chemical equation. It represents the proportions of reactants and products involved in a chemical reaction. For example, in the reaction:
  • 3 moles of hydrogen (H2) react with 1 mole of nitrogen (N2) to produce 2 moles of ammonia (NH3).
This means for every 2 units of ammonia formed, 3 units of hydrogen and 1 unit of nitrogen are needed. Mole ratios help in solving problems related to the amounts of substances consumed or produced in a reaction.
To apply mole ratio in calculations, you can set up a proportion based on the balanced equation. This allows you to calculate the unknown quantity if you have one known quantity related to the substances involved. This method was used in calculating the moles of H2 and N2 consumed.
Balanced Chemical Equation
A balanced chemical equation is a fundamental tool in chemistry. It not only represents what happens in a reaction but also ensures the law of conservation of mass is adhered to. This law states that matter cannot be created or destroyed.
In simple terms, atoms and molecules present at the start of a reaction must still be present at the end of it. Thus, a balanced equation has the same number of each type of atom on both sides of the reaction. In the ammonia synthesis equation:
  • 3H2(g)+N2(g)2NH3(g)
This equation shows that three molecules of hydrogen gas react with one molecule of nitrogen gas to form two molecules of ammonia. Balancing an equation is crucial for accurate stoichiometric calculations. Without it, determining the correct mole ratios would be impossible. Always ensure the chemical equation is balanced before performing calculations.
Ammonia Synthesis
Ammonia synthesis, often carried out through the Haber-Bosch process, is a vital industrial chemical reaction. This process is crucial for producing ammonia, a key ingredient in fertilizers that supports agricultural productivity worldwide.
The reaction involves nitrogen from the air and hydrogen derived from natural gas or water electrolysis. The balanced equation for ammonia synthesis is:
  • 3H2(g)+N2(g)2NH3(g)
This synthesis requires high temperatures and pressures to achieve significant conversion rates of nitrogen and hydrogen into ammonia. The process is designed to ensure optimal reactor efficiency while minimizing energy consumption. Understanding the stoichiometry of this reaction helps optimize conditions and calculate the necessary reactant quantities for desired product amounts.
Chemical Reaction
A chemical reaction involves rearrangement of molecules to form new substances. It is a process characterized by the interaction of reactants to form products with different properties. In the context of the ammonia synthesis reaction:
  • Hydrogen (H2) and nitrogen (N2) interact to form ammonia (NH3).
Chemical reactions can be exothermic or endothermic. Ammonia synthesis is exothermic, releasing energy due to the formation of strong nitrogen-hydrogen bonds in ammonia. Analysis of chemical reactions involves understanding changes at the molecular level, usually afforded by a balanced equation.
These reactions are central to various industries, including agriculture, pharmaceuticals, and environmental management. Knowing how reactions work allows chemists and engineers to manipulate them for desired outcomes, including the design of sustainable processes and resources.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The depletion of ozone (O3) in the stratosphere has been a matter of great concern among scientists in recent years. It is believed that ozone can react with nitric oxide (NO) that is discharged from high-altitude jet planes. The reaction is O3+NOO2+NO2 If 0.740 g of O3 reacts with 0.670 g of NO, how many grams of NO2 will be produced? Which compound is the limiting reactant? Calculate the number of moles of the excess reactant remaining at the end of the reaction.

Propane (C3H8) is a minor component of natural gas and is used in domestic cooking and heating. (a) Balance the following equation representing the combustion of propane in air: C3H8+O2CO2+H2O (b) How many grams of carbon dioxide can be produced by burning 3.65 mol of propane? Assume that oxygen is the excess reactant in this reaction.

The atomic mass of element X is 33.42 amu. A 27.22g sample of X combines with 84.10 g of another element Y to form a compound XY. Calculate the atomic mass of Y.

Each copper(II) sulfate unit is associated with five water molecules in crystalline copper(II) sulfate pentahydrate (CuSO45H2O). When this compound is heated in air above 100C, it loses the water molecules and also its blue color: CuSO45H2OCuSO4+5H2O If 9.60 g of CuSO4 is left after heating 15.01 g of the blue compound, calculate the number of moles of H2O originally present in the compound.

Analysis of a metal chloride XCl3 shows that it contains 67.2 percent Cl by mass. Calculate the molar mass of X, and identify the element.

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free