Consider the following reaction: 4NH3(g) + 502(g) – 4NO(g) + 6H2O(g); AH = -906 kJ Now...
Consider the following reaction: 6NO(g) + 4NH3(g) → 5N2(g) + 6H2O(g) ; ΔH = -1805 kJ Now answer the following two questions. 1.Which condition will release more heat? A. Combining 5.0 g of NO with excess NH4 or B. Combining 2.5 g of NH3 with excess NO 2. How much heat will be released from your answer in question 1?
Ammonia reacts with oxygen according to the equation: 4NH3(g) +502(g) → 4NO(g) + 6H2O(g) AH.,.. = 4906 kJ Calculate the heat (in kJ) associated with the complete reaction of 355 g of NH3. Express your answer with the appropriate units. Value Units
Consider the following reaction: 4NH3 + 502 --> 4NO + 6H2O. In an experiment, 3.25 g of NH3 are allowed to react with 3.50 g of 02. Only 0.490 g of NO is actually produced. What is the percent yield of NO?
Ammonia reacts with oxygen according to the equation: ANH3(g) +502(g) → 4NO(g) + 6H2O(g) AH.. = --906 kJ Calculate the heat (in kJ) associated with the complete reaction of 305 g of NH3 Express your answer with the appropriate units.
Consider the reaction 4NH3(g) +502(9) +4NO(g) + 6H2O(9) for which AH° = -905.2 kJ and A Sº = 180.5 JK at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.669 moles of NH3(g) react under standard conditions at 298.15 K. = A Suniverse JK (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the...
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
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
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
Consider the reaction: 4NH3() +502(X) -4NO() + 6H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.00 moles of NH3(e) react at standard conditions. AS system JAK
. 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?