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
The concept used to solve the given problem is the knowledge of balanced equation and stoichiometry.
Stoichiometry is the factor which ensures that the chemical equation is balanced or not. This can be used to determine energy associated to chemical species.
Stoichiometry is the relative quantities of reactant and products in chemical reactions which relates the total mass of reactant to the products.
(1)
The given reaction when ammonia reacts with oxygen is as follows:
From the balanced equation, it shows that 4 mol of reacts with of to give of and of with the complete reaction.
One mole of contains of gas. So, of contains of gas.
As the heat liberated for the or of gas is .
So, heat liberated for 1 will be as follows:
So, the heat liberated for of gas will be as follows:
(2.1)
The given reaction when butane reacts with oxygen is as follows:
From the given balanced equation, it shows thatof reacts with of to give of and of with the complete reaction.
One mole of contains of gas.
As the heat liberated for the or of gas is .
So, heat liberated for y mol is or .
So, y will be
Now, mass of butane is calculated by formula as follows:
Here M is molar mass of butane and y is number of moles of butane.
Substitute for y and for M.
(2.2)
One mol of butane gas forms of .
So, of butane will produce of . Here x is calculated as follows:
Now, mass of is calculated by formula as follows:
Here M is molar mass of butane and x is number of moles of butane.
Substitute for x and for M.
Ans: Part 1The heat associated with the complete reaction of of is .
Concepts and reason
The concept used to solve the given problem is the knowledge of balanced equation and stoichiometry.
Stoichiometry is the factor which ensures that the chemical equation is balanced or not. This can be used to determine energy associated to chemical species.
Fundamentals
Stoichiometry is the relative quantities of reactant and products in chemical reactions which relates the total mass of reactant to the products.
(1)
The given reaction when ammonia reacts with oxygen is as follows:
From the balanced equation, it shows that 4 mol of reacts with of to give of and of with the complete reaction.
One mole of contains of gas. So, of contains of gas.
As the heat liberated for the or of gas is .
So, heat liberated for 1 will be as follows:
So, the heat liberated for of gas will be as follows:
(2.1)
The given reaction when butane reacts with oxygen is as follows:
From the given balanced equation, it shows thatof reacts with of to give of and of with the complete reaction.
As the heat liberated for the or of gas is .
So, heat liberated for y mol is or .
So, y will be
Now, mass of butane is calculated by formula as follows:
Here M is molar mass of butane and y is number of moles of butane.
(2.2)
One mol of butane gas forms of .
So, of butane will produce of . Here x is calculated as follows:
Now, mass of is calculated by formula as follows:
Here M is molar mass of butane and x is number of moles of butane.
Ans: Part 1
1. Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat...
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
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
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.
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ---> 4NO + 6H2O When 20.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent? A) NO B) O2 C) H2O D) no reagent is limiting E) NH3 What is the coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced? ___C7H14 + ___ O2 ---> ___ CO2 + __ H2O A) none of these B) 10...
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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?
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 following reaction: 4NH3(g) + 502(g) – 4NO(g) + 6H2O(g); AH = -906 kJ Now answer the following two questions. 1. Which condition will release more heat? A. Combining 4.0 g of NH3 with excess O2 or B. Combining 5.0 g of O2 with excess NH3 2. How much heat will be released from your answer in question 1? Condition will release more heat and the value of this heat energy is
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the percent yield of the reaction
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