7. 4NH3(g) + 5O2(g) --------> 4NO(g) + 6H2O(g)
Keq = [NO]^4[H2O]^6/[NH3]^4[O2]^5
A. Keq = [NO]^4[H2O]^6/[NH3]^4[O2]^5
8. [H^+] = 2.5*10^-4 M
PH = -log[H^+]
= -log2.5*10^-4
= 3.6020
A. 3.6
9. H3PO4 + H2O ------> H3O^+
+ H2PO4^-
Acid1
Base2 conjugate acid2 conjugate
base1
H3PO4 and H2PO4^ are conjugate acid- base pair
C. H3Po4- H2Po4^-
10.Kinetic energy is directley proportinal to absolute
temperature.
D. The kinetic energy of gas particles does not change with
increasing temperature.
7. The equilibrium constant expression for 4 NH3(g) + 5 O2(g) + heat → 4 NO(g)...
4. Consider the reaction: 2 SO2(g) + O2(g) 3 2 SO:(g) A 2.0 L flask was filled with 0.0400 moles of SO, and 0.0200 moles of O2. At equilibrium 0.0296 moles of SO, were found. What is the equilibrium constant for this reaction? A) 2.556 x 10 B) 3.664 x 10 C) 6.953 x 102 D) 9.964 x 102 E) 3.116 x 10 5. What is a conjugate acid-base pair for the following equilibrium? H2O(l) + HSO4 (aq) = H2SO4(aq)...
Consider the following reaction: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) A scientist adds 9.00 atm of NH3(g) and 7.00 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.
7. 4 NH3 + 5 O2 ---> 4 NO + 6 H2O If 20.0 g of NH3 reacts with 20.0 g of O2, then how many grams of H2O will be made? (Answer to three sig figs. You don't need to type in the label.)
7. 4 NH3 + 5 O2 ---> 4 NO + 6 H2O If 20.0 g of NH3 reacts with 20.0 g of O2, then how many grams of H2O will be made? (Answer to three sig figs. You don't need to type in the label.
For the reaction 4 NH3(g) + 5 O2(g) \longrightarrow 4 NO(g) + 6 H2O(g), if the rate of change of NH3 ([NH3]/t) is -2.6 x 10-3 M/s at a particular time. What is rate of the reaction at the same time?
What is the equilibrium constant expression for the following reaction? 2 N 2O 5( g) 4 NO 2( g) + O 2( g) Keq = [NO2]4 [O2]2 / [N2O5]2 Keq = [N2O5]2 / [NO2]4 [O2]2 Keq = [N2O5]2 / [NO2]4 [O2] Keq = [NO2]4 [O2] / [N2O5]2 none of the above
1. For the balanced chemical reaction: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(ℓ), how many moles of H2O are produced when 0.669 mol of NH3 react? 2.For the balanced chemical reaction: 4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g) determine the number of moles of each of the products that are formed when 6.88 mol of KO2 react. Please explain, thanks!
Consider the reaction: 4 NH3 + 5 O2 4 NO + 6 H2O. The initial rate of consumption of NH3 is –1.4 × 10–5 M/s. Calculate the initial rate of production of H2O. 6. Consider the reaction: 4 NH3 + 5 02 +4 NO + 6 H20. The initial rate of consumption of NH3 is -1.4 x 10-5M/s. Calculate the initial rate of production of H20.
16. (17 points) Consider the following balanced redox reaction: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) a. Give the oxidation state of each element in the following compounds: NH3(g): N H O2(g): o NO(g): H2O(g): b. What is the oxidizing agent? c. Whatis the reducing agent? d. In one experiment, 157 g NO was recovered and the yield was determined to be 29.5%. What mass of ammonia was reacted with excess oxygen in this experiment? (MW...
10. A study of the system, 4 NH3(g) + 7 O2(g) 2 N2O4(q) + 6 H2O(g), was carried out. A system was prepared with (NH3) = [02] = 3.60 M as the only components initially. At equilibrium. [N204) is 0.60 M. Calculate the equilibrium concentration of O2. a, 3.00 M b. 2.40 M c. 1.50 M d. 2.10 M e. 3.30 M 11. For the reaction, 2 SO2(g) + O2(g) 2 SO.(a), at 450.0 K the equilibrium constant, Kc, has...