Question

In: Chemistry

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O ∆Hrxn = -906 kJ A)...

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O ∆Hrxn = -906 kJ A) Calculate the heat (in kJ) associated with the complete reaction of 0.127 Kg of NH3. B) What mass of O2 (g) is required to evolve 4605 kJ of energy

Expert Solution

mass of NH3 = 0.127 kg = 127g

moles = mass / molar mass

= 127 / 17

= 7.47

moles of NH3 = 7.47

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O ∆Hrxn = -906 kJ

4 mol of NH3 gives --------------- -906 kJ

7.47 mol NH3 ----------------- ??

heat energy = 7.47 x - 906 / 4 = -1692 kJ

heat energy = - 1692 kJ

B)

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O ∆Hrxn = -906 kJ

5 mol of O2 gives ------------------ ∆Hrxn = -906 kJ

?? mol O2 ---------------- 4605 kJ

moles of O2 = 25.41 moles

moles = mass / molar mass

25.41 = mass / 32

mass of O2 required = 813.2g

queen_honey_blossom answered 9 months ago

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) A scientist adds 7.00 atm...

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) A scientist adds 7.00 atm of NH3(g) and 8.00 atm of O2(g) to a 5.0 L container at 473 K. What will the pressure of H2O(g) be if the reaction goes to completion? Assume that the temperature remains constant. Select one: a. 6.40 atm b. 9.60 atm c. 10.5 atm d. 0.90 atm e. 15.0 atm

2C2H2 (g) + 5 O2 (g) ---------> 4 CO2 (g) + 2 H2O (g) + heat...

2C2H2 (g) + 5 O2 (g) ---------> 4 CO2 (g) + 2 H2O (g) + heat 3. Which of the following is true about reaction when the concentration of O2 (g) is decreased? a. Equilibrium will shift to the left. b. Equilibrium will shift to the right. c. No effect on the equilibrium. d. Equilibrium constant will decrease. 4. Which of the following is true about reaction when the temperature is increased? a. Equilibrium will shift to the left. b....

consider the following reaction at equilibrium: 4 NH3 + 5 O2 <---> 4 NO + 6...

consider the following reaction at equilibrium: 4 NH3 + 5 O2 <---> 4 NO + 6 H2O. What would happen to the position of the equilibrium if: a) more oxygen is added b) the pressure was increased

1. When H2(g) reacts with O2(g) to form H2O(g) , 242 kJ of energy are evolved...

1. When H2(g) reacts with O2(g) to form H2O(g) , 242 kJ of energy are evolved for each mole of H2(g) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If...

PART I - Synthesis and purification of [Cu(NH3)4]SO4.H2O Compound Mass (g) CuSO4.H2O 5.090 g [Cu(NH3)4]SO4.H2O 1.880...

PART I - Synthesis and purification of [Cu(NH3)4]SO4.H2O Compound Mass (g) CuSO4.H2O 5.090 g [Cu(NH3)4]SO4.H2O 1.880 g 1. limiting reagent determination (use the stoichiometric ratio to determine the limiting reactant) CuSO4.5H2O (s) + 4NH3 (aq) → [Cu(NH3)4]SO4.H2O (aq) + H2O (l) 2. percentage yield of crude product (remember to include the 0.025 g of compound you take for determining the absorption spectrum). PART II - Spectrophotometric analysis of the coordination complex Compound Quantity Complex mass (g) 0.026 g Volume of...

The reaction of CH3OH(g) with N2(g) to give HCN(g), NH3(g), and O2(g) requires 164 kJ/mol of...

The reaction of CH3OH(g) with N2(g) to give HCN(g), NH3(g), and O2(g) requires 164 kJ/mol of CH3OH(g). a) Write a balanced chemical equation for this reaction. Include the phases of all species in the reaction. b)Should the thermal energy involved be written as a reactant or as a product? c) How much heat is involved in the reaction of 70.0 g of CH3OH(g) with excess N2(g) to give HCN(g) and NH3(g) in this reaction?

1.) Given the following data: C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l) ΔH= -1300.kJ C(s) +...

1.) Given the following data: C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l) ΔH= -1300.kJ C(s) + O2(g) àCO2(g) ΔH= -394kJ H2(g) + O2(g) à H2O(l) ΔH= -286kJ Use Hess’s Law to calculate ΔH for the reaction 2C(s) + H2(g) àC2H2(g) 2.) Calculate ΔH° for each of the following reactions using the data for the enthalpy of formation in the appendix. 2Na(s) + 2H2O(l)à2NaOH(aq) + H2(g

2 NH3 (g) + 2 H2O (g) = 2 NO (g) + 5 H2 (g) When...

2 NH3 (g) + 2 H2O (g) = 2 NO (g) + 5 H2 (g) When 12.0 grams of ammonia; 16.0 grams of water; and 20 grams of NO (g) are put into a closed, expandable container kept at 160 oC, 1.0 atm, final partial pressure of NO (g) is 20 % greater than the final partial pressure of the hydrogen gas. What is the final volume of the expandable container? (Answer = 98.1 Liters )

2 H2O (g) + 2 Cl2 (g) + heat ----------> 4 HCl (g) + O2 (g)...

2 H2O (g) + 2 Cl2 (g) + heat ----------> 4 HCl (g) + O2 (g) 3. Which of the following is true about reaction when O2 (g) is added to the mixture. a. Equilibrium will shift to the left. b. Equilibrium will shift to the right. c. No effect on the equilibrium. d. Equilibrium constant will decrease. 4. Which of the following is true about reaction when the pressure is increased by the addition of an inert gas? a....

Consider the balanced chemical reaction shown below. 4 PH3(g) + 8 O2(g) 6 H2O(l) + 1...

Consider the balanced chemical reaction shown below. 4 PH3(g) + 8 O2(g) 6 H2O(l) + 1 P4O10(s) In a certain experiment, 3.382 g of PH3(g) reacts with 8.377 g of O2(g). (a) Which is the limiting reactant? (b) How many grams of H2O(l) form? (c) How many grams of P4O10(s) form? (d) How many grams of the excess reactant remains after the limiting reactant is completely consumed?