Isobars and Isotopes

Q. Calculate the molarity of a solution containing $5g\text{of}NaOH\text{in}450mL$ solution.

Q. Calculate the molarity of each of the following solutions:

$A$: $30g\text{of}Co(N{O}_3{)}_2.6H_{2}O\text{in}4.3L$ of solution.

$B$: $30mL\text{of}0.5M{H}_{2}S{O}_4$ diluted to $500mL$.

Q. One mole of any substance contains $6.022\times {10}^{23}$ atoms/molecules. Number of molecules of $H_{2}S{O}_4$ present in 100 mL of 0.02M $H_{2}S{O}_4$ solution is ___.

1. $12.044\times {10}^{20}$ molecules
2. $1\times {10}^{23}$ molecules
3. $12.044\times {10}^{23}$ molecules
4. $6.022\times {10}^{23}$ molecules

Q. Which of the following species is not isoelectronic with the others?

1. $N{a}^{+}$
2. $M{g}^{2+}$
3. $O^{2-}$
4. $C{l}^{-}$

Q. Assertion (A) : One atomic mass unit is defined as one twelfth of the mass of one carbon-12 atom.

Reason (R) : Carbon-12 isotope is the most abundant isotope of carbon and has been chosen as standard

1. Both A and R are false.
2. Both A and R are true and R is the correct explanation of A.
3. Both A and R are true but R is not the correct explanation of A
4. A is true but R is false.

Q.

Equivalent mass of calcium in calcium carbonate is _______________.

Q. Many elements have non-integral atomic masses because

1. They have isotopes
2. Their isotopes have non-integral masses
3. Their isotopes have different masses
4. None of these

Q.

Write the drawbacks in Mendeleev's periodic table that led to its modification.

Q.

Give the value for the following:

amount of sodium in 1 mole of sodium

Q.

what is a spherical node

Q.

Calculate the number of moles in $128g$ of $S{O}_2$ :

1. 1mole

2. 2 mole

3. $3mole$

4. $4mole$

Q.

The molar mass of sulphate ion is 96 g mol ^-1. What is the meaning of this statement?

Q.

Isotopes have the same chemical properties but different physical properties. Explain.

Q.

Please help me with all the Formulas that will be used in Mole Concept that we also used in class 9 but not to a great extent. Please help me with all of the formulas of Mole Concept! ASAP😇😇

Q.

An element X, with atomic number Z and mass number A, is represented as ${}_{\mathrm{A}}{}^{\mathrm{Z}}\mathrm{X}$.

1. True
2. False

Q.

What is period 7 called?

Q. In two elements, ${}_{Z_1}^{M_1}Aand{}_{Z_2}^{M_2}B,M_1\ne M_{2}and{Z}_1\ne Z_2\text{but}(M_1-Z_1)=(M_2-Z_2).$
A and B are:

1. Isotones
2. Isobars
3. Isotones
4. Isodiaphers

Q. The sum of the number of electrons, protons and neutrons in the three isotopes ${(}^{12}C{,}^{13}C{,}^{14}C)$ of carbon is:

1. 36
2. 18
3. 57
4. 39

Q.

The mass of one atom of chlorine is

1. $\frac{1}{6.022\times {10}^{23}}g$

2. $\frac{71}{6.022\times {10}^{23}}g$

3. $\frac{35.5}{6.022x{10}^{23}}g$

4. $71u$

Q.

Calculate the number of gram atoms in 4.6 grams of sodium $(\mathrm{N}a=23)$.

Q. The triad of nuclei that are isotonic is:

1. ${}_6^{14}C,{}_7^{15}N,{}_9^{17}F$
2. ${}_6^{12}C,{}_7^{14}N,{}_9^{19}F$
3. ${}_6^{14}C,{}_7^{14}N,{}_9^{17}F$
4. ${}_6^{14}C,{}_7^{14}N,{}_9^{19}F$

Q.

Calculate the empirical formula of a compound having $37.6\%$ sodium, $23.1\%$ silicon and $39.3\%$ oxygen.
$\left[\mathrm{O}=16,\mathrm{Na}=23,\mathrm{Si}=28\right]$

Q.

Give the relation between atomic number and atomic mass of light elements?

Q.

Calculate the number of molecules in $0.71\text{g}$ of chlorine gas. Take Avogadros number as $6\times {10}^{23}$.

Q. Determine the empirical formula of an oxide of iron, which has $69.9\%$ iron and $30.1\%$ dioxygen by mass.

Q.

Write brief notes on isobar.

Q. Which of the following species is isoelectronic with the hydride ion?

1. He
2. Be
3. $H^{+}$
4. $H{e}^{+}$

Q. Total number of electrons present in 48g ${\text{Mg}}^{\text{2+}}$ are:

1. 20 N${}_{\text{A}}$
2. 24 N${}_{\text{A}}$
3. 2 N${}_{\text{A}}$
4. None of these

Q.

Isotopes of an element have ________ chemical properties, because they have same number of _______ in their nucleus.

Q.

What is meant by the atomicity of an element? Give some examples of polyatomic elements.