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The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.?
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The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6...
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The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6...
Explanation:
First Order Decomposition: The rate of decomposition of NH4NO3 is directly proportional to the amount of NH4NO3 present. Therefore, the decomposition of NH4NO3 follows first order kinetics.
Half-Life: The half-life of a first order reaction is the time required for the concentration of the reactant to decrease to half of its initial value.
Given,
Half-life (t1/2) = 2.10 hours
We can use the following equation to calculate the rate constant (k) of the reaction.
t1/2 = (0.693/k)
k = (0.693/t1/2) = (0.693/2.10) = 0.33 hr^-1
Time Required for 90% Decomposition:
We can use the following equation to calculate the time required for 90% decomposition of NH4NO3.
ln (Co/C) = kt
Where, Co = initial concentration of NH4NO3
C = concentration of NH4NO3 at time t
Here, Co = 6.2 g (given)
C = 0.1 Co = 0.62 g (since 90% is decomposed)
Substituting the values, we get:
ln (6.2/0.62) = (0.33 t)
t = 6.978 hours
Therefore, the time required for 90% decomposition of NH4NO3 is 6.978 hours.
Volume of N2O Produced:
NH4NO3 decomposes to form N2O and H2O in the ratio of 1:2. Therefore, the moles of N2O produced can be calculated as follows:
Moles of NH4NO3 = 6.2 g / molar mass of NH4NO3
= 6.2 g / (14 + 4 + 14 + 3*16)
= 0.046 moles
Moles of N2O produced = 0.5 * moles of NH4NO3
= 0.5 * 0.046
= 0.023 moles
Using the ideal gas equation, we can calculate the volume of N2O produced at STP.
PV = nRT
Where, P = pressure = 1 atm
V = volume of N2O produced
n = moles of N2O produced
R = gas constant = 0.0821 L atm / mol K
T = temperature at STP = 273 K
Substituting the values, we get:
V = (nRT)/P
= (0.023 * 0.0821 * 273) / 1
= 1.562 L
Therefore, the volume of N2O produced at STP is 1.562 L.
First Order Decomposition: The rate of decomposition of NH4NO3 is directly proportional to the amount of NH4NO3 present. Therefore, the decomposition of NH4NO3 follows first order kinetics.
Half-Life: The half-life of a first order reaction is the time required for the concentration of the reactant to decrease to half of its initial value.
Given,
Half-life (t1/2) = 2.10 hours
We can use the following equation to calculate the rate constant (k) of the reaction.
t1/2 = (0.693/k)
k = (0.693/t1/2) = (0.693/2.10) = 0.33 hr^-1
Time Required for 90% Decomposition:
We can use the following equation to calculate the time required for 90% decomposition of NH4NO3.
ln (Co/C) = kt
Where, Co = initial concentration of NH4NO3
C = concentration of NH4NO3 at time t
Here, Co = 6.2 g (given)
C = 0.1 Co = 0.62 g (since 90% is decomposed)
Substituting the values, we get:
ln (6.2/0.62) = (0.33 t)
t = 6.978 hours
Therefore, the time required for 90% decomposition of NH4NO3 is 6.978 hours.
Volume of N2O Produced:
NH4NO3 decomposes to form N2O and H2O in the ratio of 1:2. Therefore, the moles of N2O produced can be calculated as follows:
Moles of NH4NO3 = 6.2 g / molar mass of NH4NO3
= 6.2 g / (14 + 4 + 14 + 3*16)
= 0.046 moles
Moles of N2O produced = 0.5 * moles of NH4NO3
= 0.5 * 0.046
= 0.023 moles
Using the ideal gas equation, we can calculate the volume of N2O produced at STP.
PV = nRT
Where, P = pressure = 1 atm
V = volume of N2O produced
n = moles of N2O produced
R = gas constant = 0.0821 L atm / mol K
T = temperature at STP = 273 K
Substituting the values, we get:
V = (nRT)/P
= (0.023 * 0.0821 * 273) / 1
= 1.562 L
Therefore, the volume of N2O produced at STP is 1.562 L.
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The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.?
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The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.?.
The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The half life of a first order decomposition of NH4NO3 is 2.10hr. If 6.2g of NH4NO3 is allowed to decompose the time required for decomposition of 90%NH4NO3 and the volume of dry N20 produced at this point at STP.?Answer is 6.978hr and 1.562L.?.
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