Answer:
Compound Interest is calculated on the initial Principal for a given unit of time(yearly, half-yearly, quarterly), it also includes all of the accumulated interests of the previous period of a loan or deposit.
In this type of interest, the amount after the first unit time becomes the principal for the second unit and the amount after second unit time becomes the principal for the third unit and so on.
So the difference between the final amount and the principal is called Compound interest.
If the interest is compounded yearly:-
A=P(1+R100)n
Here A = final Amount
P = Principal
R = interest rate
n = time period
Compound interest = Final amount - principal
Given:-
Principal (P) = $4000
Interest Rate (R) = 6%
Time period (n) = 5 years
Answer:
Explanation: The lowest pressure in a laboratory is 4.0×10^-11Pa
Using Ideal gas equation
PV = nRT
P= 4.0×10^-11Pa
V= 0.020m^3
T= 20+273= 293k
n=number of moles = m/A
Where m is the number of molecules and A is the Avogradro's number=6.02×10²³/mol
R=8.314J/(mol × K)
PV= m/A(RT)
4.0×10^-11 ×0.020 = m/6.02×10²³(8.314×293)
m = 4.0×10^-11×0.020×6.02×10^23 / (8.314×293)
m = 1.98×10^8 molecules
Therefore,the number of molecules is 1.98×10^8
Mass = Density x Volume
Mass = 3.2g/mL x 5 mL
Mass = 16g
Answer:
a) equivalence point
b) direct titration
c) primary standard
d) titrand
e) Back titration
f) back titration
g) standard solution
h) standard solution
I) indirect titration
j) end point
Explanation:
A volumetric analysis is one in which a solution of unknown concentration is determined from its volume. This is commonly referred to as titration.
In titration, a standard solution is reacted with another solution of unknown concentration. The point at which the concentration of the standard solution is equal to that of the analyte is known as the equivalence point (usually indicated by a colour change). An indicator may be added to the analyte solution to help identify when the reaction is complete.
Explanation:
20.0 moles= 80.1 or 80.05g
5.00 moles= 20.0g
1.20×1025moles= 4923.2g
1.00 moles= 4.00g
80.0 moles= 320.2g
