Nitrogen Fixation N2 + 3H2 → 2NH3 Nitrification 2NH3 + 302 → 2NO2 + 2H2O+2H+ Denitrification 2NO3 + 2CH2O + 2H* → N20 + 2CO2 + 3H2O The table above shows the balanced chemical equations that represent three processes that are part of the nitrogen cycle. Which of the following is exemplified by the equations above? (A Approximately 10% of energy is transferred from one trophic level to the next. (B In a food web, energy flows and matter is cycled. Each biogeochemical cycle demonstrates the conservation of matter. D) The major reserve for nitrogen is in the atmosphere.

Nitrogen Fixation N2 + 3H2 → 2NH3 Nitrification 2NH3 + 302 → 2NO2 + 2H2O+2H+ Denitrification 2NO3 + 2CH2O + 2H* → N20 + 2CO2 + 3H2O The table above shows the balanced chemical equations that represent three processes that are part of the nitrogen cycle. Which of the following is exemplified by the equations above? (A Approximately 10% of energy is transferred from one trophic level to the next. (B In a food web, energy flows and matter is cycled. Each biogeochemical cycle demonstrates the conservation of matter. D) The major reserve for nitrogen is in the atmosphere.

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

How many grams of water will be produced when 26.00 g of glucose reacts with 26.00 g of oxygen?
How many grams of Cl2 can be prepared from the reaction of 8.0 g of MnO2 and 30.0 g of HCl according to the following balanced chemical equation? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
What are the resulting products formed when LiBr reacts with F2 in a Single Replacement Reaction?
If you wanted to produce 4 moles of SO3 gas, how many moles of SO2 would you need to react? (Assume an unlimited supply of O2 gas.) 2 SO₂ (g) + O₂(g) →2 SO, (g)
Use the chemical equation below to determine how many moles of ammonia will be produced from 4 moles of nitrogen gas. Assume that there is enough H2 for all of the N2 to be converted to NH3. N2 + 3H2 ---> 2NH3
A 6.79 g sample of NH, gas and a 6.79 g sample of HCl gas are mixed in a 1.50 L flask at 25 °C. < EFeedback You have not correctly determined the mass of NH,Cl formed. Identify the limiting reagent. Convert the given mass of the limiting reagent to the mass of NH,Cl using the NH; mole ratio from the balanced chemical HCI equation and the molar masses for both NH,CI the limiting reagent and the NH,Cl as conversion factors. How many grams of NH,Cl will be formed by this reaction? 0.273 mass: Incorrect What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH,Cl produced by the reaction. P = 3.42
Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. C(s) + H, (g) → C,H, (g)
How many moles of H2O2 are needed to produce 3.90 mol of H2O?
Hydrochloric acid is reacted with iron (II) sulfide to form hydrogen sulfideLinks to an external site. according to the balanced chemical equation. If 1.52 mols of hydrochloric acid are reacted with 1.22 mols of iron (II) sulfide, how many mols of hydrogen sulfide are formed?
ise. Question 10 When the following equation is balanced, the coefficient of H 1 is Al (S) + H 20 (1) → Al(OH) 3 (S) + H 2 (g) 0 1 O 2 O 4 O 3 O 5 A Moving to another question will save this response.
Balance the following the chemical equation
Balance the following chemical equation (if necessary): NH3(g) + O₂(g) → NO(g) + H₂O(g) -