Fundamentals Of Chemistry In Biological Systems Practice Tests

Question 1

An element has an atomic number of 17 and a mass number of 35. Calculate the number of neutrons in the nucleus of this atom.

Accepted Answer

18

Question 2

If a neutral atom of an element loses two electrons to form a stable ion, what is the resulting charge of the ion?

Accepted Answer

+2

Answer

-2

Answer

+1

Answer

0

Question 3

Consider an isotope with 6 protons, 8 neutrons, and 6 electrons. If this isotope undergoes radioactive decay and loses one neutron, what is the new mass number of the atom?

Accepted Answer

13

Answer

12

Answer

14

Answer

15

Question 4

In a water molecule ($H_2O$), the oxygen atom exerts a stronger pull on shared electrons than the hydrogen atoms, creating a polar covalent bond.

Accepted Answer

True

Answer

False

Question 5

Which of the following scenarios describe a chemical change rather than a physical change?

Answer

Chopping wood into smaller pieces

Answer

Burning a piece of wood

Answer

Melting an ice cube

Answer

Digesting a protein molecule

Question 6

If a sodium atom (atomic number 11) transfers an electron to a chlorine atom (atomic number 17), determine the resulting electron configuration of the sodium ion ($Na^+$) in terms of total electrons.

Accepted Answer

10

Question 7

Given that carbon has 4 valence electrons and requires 8 for a stable shell, how many single covalent bonds must a carbon atom form to achieve stability?

Accepted Answer

4

Answer

2

Answer

3

Answer

8

Question 8

A patient presents with a blood pH of $7.20$. Given that $pH = -\log_{10}[H^+]$, calculate the concentration of hydrogen ions $[H^+]$ in the patient's blood in $mol/L$.

Accepted Answer

6.31 	imes 10^{-8} mol/L

Question 9

If a solution's pH changes from $4.0$ to $2.0$, by what factor does the concentration of hydrogen ions $[H^+]$ increase?

Accepted Answer

Option A

Answer

Option B

Answer

Option C

Answer

Option D

Question 10

Determine the mass of $NaOH$ (molar mass $40.0 g/mol$) required to completely neutralize $500 mL$ of $0.1 M$ $HCl$ solution according to the reaction $HCl + NaOH \rightarrow H_2O + NaCl$.

Accepted Answer

2.0 g

Question 11

A blood pH of $7.50$ indicates that the patient is in a state of acidosis.

Accepted Answer

False

Answer

True

Question 12

Which of the following ions are primary contributors to maintaining fluid balance and electrical conductivity in the human body?

Accepted Answer

Option A

Answer

Option B

Answer

Option C

Answer

Option D

Question 13

Calculate the final pH of a solution if $0.01$ moles of $HCl$ are added to $1 L$ of pure water (assume volume remains constant and $HCl$ dissociates completely).

Accepted Answer

2

Question 14

In the neutralization reaction $HCl + NaOH \rightarrow H_2O + NaCl$, what is the net ionic equation?

Accepted Answer

Option A

Answer

Option B

Answer

Option C

Answer

Option D

Question 15

If the hydrolysis of one mole of ATP releases $30.5	ext{ kJ/mol}$ of energy, calculate the total energy released in $	ext{kJ}$ when $0.25	ext{ moles}$ of ATP are consumed by a muscle cell.

Accepted Answer

7.625 kJ

Question 16

A clinical solution contains $50	ext{ g}$ of glucose dissolved in $500	ext{ mL}$ of water. If the density of the final solution is $1.1	ext{ g/mL}$, determine the concentration of the solute in terms of mass percentage ($\frac{	ext{mass of solute}}{	ext{mass of solution}} 	imes 100$).

Accepted Answer

8.33%

Answer

9.09%

Answer

10.00%

Answer

5.00%

Question 17

In a precipitation reaction where $A + B 	o C(s)$, if the concentration of ions exceeds the solubility product constant $K_{sp}$, a solid precipitate will form.

Accepted Answer

True

Answer

False

Question 18

Which of the following scenarios describe a mixture that would be classified as a suspension rather than a true solution?

Answer

Large particles that settle at the bottom of a container over time

Answer

A mixture where the particles are visible to the naked eye and can be filtered out

Answer

A homogeneous mixture where light passes through without scattering

Answer

A mixture where solute particles are smaller than $1	ext{ nm}$

Question 19

A patient is administered a medication that reacts with blood plasma to form a precipitate. If the reaction rate is defined by $R = k[A][B]$, and the initial concentrations are $[A] = 0.02	ext{ M}$ and $[B] = 0.03	ext{ M}$ with a rate constant $k = 5.0	ext{ M}^{-1}	ext{s}^{-1}$, calculate the initial reaction rate $R$ in $	ext{M/s}$.

Accepted Answer

0.003 M/s

Question 20

If the energy required to synthesize ATP from ADP and inorganic phosphate is $30.5	ext{ kJ/mol}$, and a metabolic process provides $150	ext{ kJ}$ of energy with an efficiency of $40\%$, how many moles of ATP can be synthesized?

Accepted Answer

1.97 moles

Answer

4.92 moles

Answer

2.50 moles

Answer

0.51 moles

Fundamentals Of Chemistry In Biological Systems Practice Tests

Practice Tests

Fundamentals of Chemistry in Biological Systems

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