Answer:
6.88 mg
Explanation:
Step 1: Calculate the mass of ³²P in 175 mg of Na₃³²PO₄
The mass ratio of Na₃³²PO₄ to ³²P is 148.91:31.97.
175 mg g Na₃³²PO₄ × 31.97 g ³²P/148.91 g Na₃³²PO₄ = 37.6 mg ³²P
Step 2: Calculate the rate constant for the decay of ³²P
The half-life (t1/2) is 14.3 days. We can calculate k using the following expression.
k = ln2/ t1/2 = ln2 / 14.3 d = 0.0485 d⁻¹
Step 3: Calculate the amount of P, given the initial amount (P₀) is 37.6 mg and the time elapsed (t) is 35.0 days
For first-order kinetics, we will use the following expression.
ln P = ln P₀ - k × t
ln P = ln 37.6 mg - 0.0485 d⁻¹ × 35.0 d
P = 6.88 mg
<u>Answer: </u>The correct answer is Option B.
<u>Explanation:</u>
First law of thermodynamics states that the energy can neither be destroyed not be formed but it can only be transformed from one form to another.
Here, the internal energy of the system is being transformed to the heat energy and the work done by the system. The equation used to represent first law of thermodynamic is:
where,
represents the internal energy of the system.
Q = heat released or absorbed by the system.
w = work done by or on the system.
Hence, the correct answer is Option B.
Answer: You know that monomers that are joined by condensation polymerization have two functional groups. You also know (from Part 6) that a carboxylic acid and an amine can form an amide linkage, jand a carboxylic acid and an alcohol can form an ester linkage.
Answer: the first option is correct
Why: the seed is the one doing all the work and no other forces were mentioned after 4 days
Answer:
Rate of reaction =
Rate of consumption of A = 
Rate of consumption of B =
Rate of formation of D = 
Explanation:
According to laws of mass action for the given reaction,
![Rate= -\frac{1}{2}\frac{\Delta [A]}{\Delta t}=-\frac{\Delta [B]}{\Delta t}=\frac{1}{2}\frac{\Delta [C]}{\Delta t}=\frac{1}{3}\frac{\Delta [D]}{\Delta t}](https://tex.z-dn.net/?f=Rate%3D%20-%5Cfrac%7B1%7D%7B2%7D%5Cfrac%7B%5CDelta%20%5BA%5D%7D%7B%5CDelta%20t%7D%3D-%5Cfrac%7B%5CDelta%20%5BB%5D%7D%7B%5CDelta%20t%7D%3D%5Cfrac%7B1%7D%7B2%7D%5Cfrac%7B%5CDelta%20%5BC%5D%7D%7B%5CDelta%20t%7D%3D%5Cfrac%7B1%7D%7B3%7D%5Cfrac%7B%5CDelta%20%5BD%5D%7D%7B%5CDelta%20t%7D)
where, ![-\frac{\Delta [A]}{\Delta t}](https://tex.z-dn.net/?f=-%5Cfrac%7B%5CDelta%20%5BA%5D%7D%7B%5CDelta%20t%7D)
is rate of consumption of A, ![-\frac{\Delta [B]}{\Delta t}](https://tex.z-dn.net/?f=-%5Cfrac%7B%5CDelta%20%5BB%5D%7D%7B%5CDelta%20t%7D)
is rate of consumption of B, ![\frac{\Delta [C]}{\Delta t}](https://tex.z-dn.net/?f=%5Cfrac%7B%5CDelta%20%5BC%5D%7D%7B%5CDelta%20t%7D)
is rate of formation of C and ![\frac{\Delta [D]}{\Delta t}](https://tex.z-dn.net/?f=%5Cfrac%7B%5CDelta%20%5BD%5D%7D%7B%5CDelta%20t%7D)
is rate of formation of D
Here ![\frac{\Delta [C]}{\Delta t}=2.7mol.dm^{-3}.s^{-1}](https://tex.z-dn.net/?f=%5Cfrac%7B%5CDelta%20%5BC%5D%7D%7B%5CDelta%20t%7D%3D2.7mol.dm%5E%7B-3%7D.s%5E%7B-1%7D)
So, Rate of reaction = 
Rate of formation of D = ![(\frac{3}{2}\times \frac{\Delta [C]}{\Delta t})=(\frac{3}{2}\times 2.7mol.dm^{-3}.s^{-1})=4.15mol.dm^{-3}.s^{-1}](https://tex.z-dn.net/?f=%28%5Cfrac%7B3%7D%7B2%7D%5Ctimes%20%5Cfrac%7B%5CDelta%20%5BC%5D%7D%7B%5CDelta%20t%7D%29%3D%28%5Cfrac%7B3%7D%7B2%7D%5Ctimes%202.7mol.dm%5E%7B-3%7D.s%5E%7B-1%7D%29%3D4.15mol.dm%5E%7B-3%7D.s%5E%7B-1%7D)
Rate of consumption of A = ![(\frac{2}{2}\times \frac{\Delta [C]}{\Delta t})=(\frac{2}{2}\times 2.7mol.dm^{-3}.s^{-1})=2.7mol.dm^{-3}.s^{-1}](https://tex.z-dn.net/?f=%28%5Cfrac%7B2%7D%7B2%7D%5Ctimes%20%5Cfrac%7B%5CDelta%20%5BC%5D%7D%7B%5CDelta%20t%7D%29%3D%28%5Cfrac%7B2%7D%7B2%7D%5Ctimes%202.7mol.dm%5E%7B-3%7D.s%5E%7B-1%7D%29%3D2.7mol.dm%5E%7B-3%7D.s%5E%7B-1%7D)
Rate of consumption of B = ![(\frac{1}{2}\times \frac{\Delta [C]}{\Delta t})=(\frac{1}{2}\times 2.7mol.dm^{-3}.s^{-1})=1.35mol.dm^{-3}.s^{-1}](https://tex.z-dn.net/?f=%28%5Cfrac%7B1%7D%7B2%7D%5Ctimes%20%5Cfrac%7B%5CDelta%20%5BC%5D%7D%7B%5CDelta%20t%7D%29%3D%28%5Cfrac%7B1%7D%7B2%7D%5Ctimes%202.7mol.dm%5E%7B-3%7D.s%5E%7B-1%7D%29%3D1.35mol.dm%5E%7B-3%7D.s%5E%7B-1%7D)
