Calculate the ^Ho in (kj) for the following reaction : 4NH3 (s) + 5O2 (g) ---> 4NO (g) + 6H2O (l)
^Ho:
NH3 - 46.0
NO 90.0
H2O - 286
A. - 1,172
B. - 1,716
C. - 150
D. - 1,356
So the enthalpy change is -1172 KJ. Negative sign represent that the energy is released.
So option 1 is correct.
Calculate the ^Ho in (kj) for the following reaction : 4NH3 (s) + 5O2 (g) --->...
Consider the following equilibrium reaction: 4NH3(g) + 5O2(g) <---> 4NO(g) + 6H2O(g) Heat = -904.4 kJ How does each of the following changes affect the yield of NO at equilibrium? Answer increase, decrease, or no change. a. increase [NH3] b. Increase [H2O] c. Decrease [O2] d. Decrease the volume of the container in which the raction occurs. e. Add a catalyst f. Increase temperature
Use standard enthalpies of formation to determine the ΔHo in kJ for the following reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) ΔHfo (NH3(g)) = -45.90 kJ/mol ΔHfo (NO(g)) = 90.29 kJ/mol ΔHfo (H2O(g)) = -241.83 kJ/mol
Consider the following reaction: 4NH3 + 5O2 4NO + 6H2O Determine the following rates at a time when the rate of consumption of O2 is 1.26e-03 M/s. a) rate of consumption of NH3 M/s b) rate of formation of NO M/s c) rate of formation of H2O M/s d) rate of reaction M/s
Part A Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat (in kJ) associated with the complete reaction of 155 g of NH3. Part B What mass of butane in grams is necessary to produce 1.5×103 kJ of heat? What mass of CO2 is produced? Assume the reaction to be as follows: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g),ΔHrxn=−2658 kJ
1. Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat (in kJ) associated with the complete reaction of 155 g of NH3. 2. What mass of butane in grams is necessary to produce 1.5×103 kJ of heat? What mass of CO2 is produced? Assume the reaction to be as follows: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g),ΔHrxn=−2658 kJ
Calculate ∆H°rxn using ∆Hf° for the reaction 4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(l ) Compound ∆H°f (kJ/mol) NH3(g) -46.0 NO2 (g) +34.0 H2O(l) -285.9
(1) Which of the following statements is correct for the equation shown here? 4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(g) (a) 6 g of H2O are produced for every 4 g of NH3 reacted. (b) 1 mole of NO is produced per mole of NH3 reacted. (c) 2 moles of NO are produced for every 3 moles of O2 reacted. (2) Silicon reacts with chromium(III) oxide according to the equation 3Si(s) + 2Cr2O3(s) ⟶ 3SiO2(s) + 4Cr(s) If 59.4 g...
Consider the reaction4NH3(g) +5O2(g) ⇌ 4NO(g)+6H2O(g) where ΔS° rxn= 180.5 J/KUsing standard thermodynamic data (in the Chemistry References), calculate the entropy change of the surroundings and the universe at 25°C.
Complete the following: a. Using standard heats of formation, determine ΔH for the following reaction: 4NH3(g) + 5O2(g) →4NO(g) + 6H2O(l) b. Estimate the difference between ΔHreaction and ΔEreaction (in kJ/mol) for the reaction: C40H80(s) + 60O2(g) →40CO2(g) + 40H2O(s) at 298 K
. Given the following reaction at 25o C. 4NH3(g) + 5 O2(g) 4NO(g) + 6H2O(l) ΔHo = -1168 kJ ΔHo f(NH3) = -46.2 kJ/mol; ΔHo f(H2O) = -285.8 kJ/mol. What is the standard enthalpy of formation of NO gas at 25o C?