Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process.In the first step, nitrogen and hydrogen react to form ammonia:N,(9)+3 H,(g)→2NH,(g)In the second step, ammonia and oxygen react to form nitric acid and water:NH3(g)+20,(9)→HNO;(g)+H,0(g)Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.

Answered: Image /qna-images/answer/fcbabf25-c046-44d3-bdbd-36d5002daf8f.jpg

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N,(g)+3 H,(g)→2 NH,(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g)+20,(g)→HNO,(g)+H,O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N,(g)+3 H,(g)→2 NH,(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g)+20,(g)→HNO,(g)+H,O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.

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

Identify the correctly written "formation reaction" among the following reactions. Hint: Recall the definition of a "formation reaction". O 2H2 (g) + 02 (g)→ 2H20 (1) N2 (g) + O2 (g) → 2NO (g) O 2H2 (g) + 02 (g)→ 2H20 (g) 2C (s. graphite) + 2H2(g) → C2H4 (g) H20 () + 1/2 02 (g) → H202 (1)
Determine how much energy in kJ is absorbed when 6.03 g of HA, the limiting reactant, are completely used in the reaction. 2 HA (s) + X(OH)2 (aq) --> XA₂ (aq) + 2 H₂O (g) AH = 647.7 kJ You may or may not need the following molar mass information: HA molar mass = 46.31 g/mol H F9 F10 F3 O D)) # 3 E D C F4 KAA णी व $ 4 R F F5 ➤ 11 V do in % 5 F6 T G A B A 6 F7 H F8 & 7 N 8 U J * 00 8 a M K €1 ( 9 O F11 Ö ) O F12 P PE
Do the follow reactions depict Heat of Formation Reactions? If so, mark the reaction as YES, if it is not a Heat of Formation Reaction, then choose NO. ✓3/2 H₂(g) + P(s) → PH3(g) H₂(g) + 1/2O₂(g) → H₂O(g) Al(s) + 3/2 Br₂(1)→ AlBr3(S) Na(s) + H₂O(1)→ NaOH(aq) + 1/2 H₂(g) ✓2As(s) + 5/2 O₂(g) → As2O5(s) In formation reactions the reactants must be elements in their most common states, and the only product is one mole of the substance of interest.
A chemist measures the enthalpy change AH during the following reaction: 2 KCl(s) + 3 0,(9)→2 KCIO 3(s) AH=78. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 3 K CI(e) + 0,«) → K CI0, (-) 0, g) 2 K C10, (s) kJ 6K C10, (s) → 6K cI (s) + 90,(g) kJ 3 2K C10, (s) 2K C1 (s) + 30,(8) I kJ
Consider the reaction below for the combustion of methane (CH4, which is the principal component of natural gas). When natural gas is combusted, heat is given off that can be used to provide warmth in homes as well as to heat water, and it is increasingly used as an alternative to coal for the production of electricity. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) + q Which of the following statements are correct? The combustion of methane is endothermic, and the sign of ∆Hrxn is negative. The combustion of methane is endothermic, and the sign of ∆Hrxn is positive. The combustion of methane is exothermic, and the sign of ∆Hrxn is positive. The combustion of methane is exothermic, and the sign of ∆Hrxn is negative.
The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application today, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H₂SO4(1)→ SO3(g) + H₂O(1) AH +113. kJ In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) + PbO₂(s) + 2SO3(g) 2 PbSO4(s) Calculate the net change in enthalpy for the formation of one mole of lead (II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ. kJ AH = -775. kJ X
Which of the following is the formation reaction for Na2CO3 (s)? A. 2 Na(s) + C(s, graphite) + 3 O(g) → Na2CO3(s) B. 4 Na(s) + 2 C(s, graphite) + 3 O2(g) → 2 Na2CO3(s) C. 2 Na(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) D. Na2(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) E. 2 Na(g) + C(g) + 1.5 O2(g) → Na2CO3(s)
Explain why each of the following chemical equations is not a correct formation reaction:(a) 4 AI(s) + 3 O2(g)→2 AI2O3(s)(b) N2(g) +3/2 H2(g) → NH3(g)(c) 2 Na(s) + O(g) → Na2O(s)
The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M acetic acid solution and 50.03 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 19.9 oC, and the final temperature after addition is 26.8 oC. What is the molar enthalpy of neutralization, in units of kJ/mol? Assume that: the calorimeter is completely insulated the heat capacity of the empty calorimeter is the heat capacity of the aluminum cup: 0.903 J g-1 oC-1. the density of the two solutions is the same as that of water: 1.00 g/mL. the heat capacity of the two solutions is the same as that of water: 4.184 J g-1 oC-1. Perform all calculations without rounding, but then provide your answer to the correct number of significant figures.
A household water heater containing 50 gallons (227 L) of water is heated burning natural gas (methane, molar mass = 16.043 g mol-1) via the following reaction: CH4(g) + O2(g) CO2(g) + H20(O A,H = -891 kJ mol-1 What mass of methane, in units of g, is needed to heat the 227 L of water in the heater from 25.0°C to 44.0°C? Assume: • the heater is 100% efficient in its use of heat energy • no heat is lost to the surroundings specific heat of water is: 4.184 Jg-1 °C-1 density of water is: 0.9970 g mL¯1
In a constant-pressure calorimeter, 70.0 mL of 0.340 M Ba(OH), was added to 70.0 mL of 0.680 M HCI. The reaction caused the temperature of the solution to rise from 24.12 °C to 28.75 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g · °C.) respectively), what is AH for this reaction (per mole H, O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,O
The reaction that was on the screen when you started and its derivative demonstrate that the reaction enthalpy, ΔH, changes sign when a process is reversed. Consider the reaction H2O(l)→H2O(g), ΔH =44.0kJ What will ΔH be for the reaction if it is reversed?