The following question refers to the reaction:
4NH3(g) + 5O2(g) ⇌ 4NO(g) + 6H2O(g)
The reaction as written is exothermic. What will happen if heat is added to the system?
(A) The equilibrium will shift to the left
(B) The equilibrium will shift to the right
(C) The NO concentration will remain constant, but there will be more water vapour
(D) The equilibrium position will not change if heat is added
(E) The system increase in temperature
Explanation will be much appreciated! Thanks in Advance
According to Le Chatelier principle, a system at equilibrium when disturbed by an external force will proceed in an opposite direction to negate the external force.
So when heat is added to the system at equilibrium, the reaction proceeds in a direction in which added heat is consumed.
Given the reaction as written is exothermic. So the backward reaction would be endothermic. Hence by adding heat backward reaction will take place to absorb the extra heat added.
Ans: (A) The equilibrium will shift to the left
The following question refers to the reaction: 4NH3(g) + 5O2(g) ⇌ 4NO(g) + 6H2O(g) The reaction...
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
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.
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
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
1. Given the balanced equation 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), if 82.0 g of NH3 react with sufficient oxygen, how many grams of NO should form? 2. Consider the reaction between sodium metal and chlorine gas to form sodium chloride (table salt): 2Na(s) + Cl2(g) → 2NaCl(s) If the mass of the sodium solid increases by 0.500 g, what mass of sodium metal should have reacted?
Enter your numbers into 1 decimal places. For the reaction: 4NO(g) + 6H2O(g) ⇋ 4NH3(g) + 5O2(g) Determine ΔH° and ΔS° for the reaction at 298 K. ΔH0(kJ) ΔS0(J/K) Assuming that these values are relatively independent of temperature, calculate ΔG° at 100.°C and 2560.°C. ΔG0(kJ)at 100℃ ΔG0(kJ) at 2560℃ 3. Is this reaction spontaneous at all range of temperature? Enter 1 for true or 0 for false. 4. Calculate the K at 298K for the above reaction. Enter "is" for...
From the following balanced equation, 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(l) how many grams of NO can be formed from 3.78g O2? Options: (a) 2.55g (b) 2.84g (c) 4.43g (d) 5.04g
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
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?