Determination of atomic and isotopic mass - class-XI
| Description: determination of atomic and isotopic mass | |
| Number of Questions: 17 | |
| Created by: Tanya Dwivedi | |
| Tags: chemistry some basic concepts of chemistry |
There are two isotopes of an element with atomic mass $z$. Heavier one has atomic mass $z+2$ and lighter one has $z-1$, then an abundance of lighter one is:
$ _{ 17 }^{ 35 }{ Cl }$ and $ _{ 17 }^{ 37 }{ Cl }$ are two isotopes of chlorine. If average atomic mass is $35.5$ then ratio of these two isotopes is:
If isotopic distribution of $ C-12 $ and $ C-14 $ is 98 % and 2 % respectively, what would be the number of $ C-14 $ isotope in $ 12 gm $ carbon sample?
Chlorine has two naturally occurring isotopes, $^{35}Cl$ and $^{37}Cl$. If the atomic mass of Cl is 35.5 the ratio of natural abundance of $^{35}Cl$ and $^{37}Cl$ is closest to :
A sample of perfect gas that initially occupies $15.0L$ at $300K$ and $1.0$ bar is compressed isothermally. To what volume must the gas be compressed to reduce its entropy by $5.0J/K$? $\left[ \ln { 0.36 } =-1.0,\ln { 2.7 } =1.0 \right] $
If an element $z$ having atomic weight $x$ exists in two isotopes of mass number $(x-1)$ and $(x+2)$ then, the percentage abundance of heavier isotopes is:
A system undergoes a process in which the entropy change is $+5.51J{K}^{-1}$. During the process, $1.50kJ$ of heat is added to the system at $300K$. The correct information regarding the process is
The table shows the numbers of particles present in the nuclei of four atoms or ions.
| protons | neutrons | electronic structure | |
|---|---|---|---|
| $1$ | $18$ | $22$ | $2, 8, 8$ |
| $2$ | $19$ | $20$ | $2, 8, 8$ |
| $3$ | $19$ | $21$ | $2, 8, 8, 1$ |
| $4$ | $20$ | $20$ | $2, 8, 8, 2$ |
Which two particles belong to the same element?
The average atomic mass of copper is $63.546$ amu .Natural copper consists of two iostopes: $^{63} Cu$ and $^{65} Cu$.Their natural abundances are $69.09\%$ and $30.91\%$ respectively. If the mass of $^{63} Cu$ isotope is $62.9298$ amu ,What is the mass of $^{65} Cu$ isotope?
Europium consists of $47.8$% Eu-$151$ and $52.2$% Eu-$153$. Calculate average atomic mass?
Rhenium (Re) consists of $37.1$% $185$ Re and $62.9$% $187$ Re. Calculate the relative atomic mass?
The relative abundance of two isotopes of atomic masses 85 and 87 are 75% and 25% respectively. The average atom mass of element is:
Antimony (Sb) is $57.2$% Sb-$121$ and $42.8$% Sb-$123$. Calculate the average atomic mass?
The relative atomic mass of an atom is:
Chromium has four stable isotopes.$4.31$% Cr-$50$, $83.76$% Cr-$52$, $9.55$% Cr-$53$ and $2.38$% Cr-$54$. Calculate the relative atomic mass?
Consider a reversible isentropic expansion of $1$ mole of an ideal monoatomic gas from ${27}^{o}C$ to ${927}^{o}C$. If the initial pressure of gas was $1$ bar, the final pressure of gas becomes
Boron found in nature has an atomic weight of 10.811 and is made up of the isotopes $\displaystyle { B }^{ 10 }$ (mass 10.013 amu) and $\displaystyle { B }^{ 11 }$ (mass 11.0093). What percentage of naturally occurring boron is made up of $\displaystyle { B }^{ 10 }$ and $\displaystyle { B }^{ 11 }$, respectively?