Medicinal Chemistry Fundamentals Quiz

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Questions and Answers

How many moles of CO2 are produced from the reaction of 856g of C6H12O6?

14.5 mol CO2

28.5 mol CO2 (correct)

18.75 mol CO2

40 mol CO2

What is the molar mass of CO2?

44.01 g/mol (correct)

28.02 g/mol

54.00 g/mol

32.00 g/mol

In a solution, which component is generally present in larger amounts?

Solvent (correct)

Solution

Chemical compound

Solute

When converting grams to moles, what is the formula used?

Moles = mass / molar mass Signup and view all the answers

What type of solution is formed when salt is dissolved in water?

Saline solution Signup and view all the answers

What is the mass of 0.356 moles of zinc in grams?

23.3 g Signup and view all the answers

How many moles are there in 3 x 10^22 atoms of gold?

0.05 mol Signup and view all the answers

What is the molecular mass of glucose in grams per mole?

180.16 g/mol Signup and view all the answers

If you have 30 g of glucose, how many moles does this represent?

0.166 mol Signup and view all the answers

Using the formula mass = number of moles x molar mass, how would you solve for the mass of a substance?

By multiplying the number of moles by the molar mass. Signup and view all the answers

What is the relationship between molar mass in g/mol and atomic mass in a.m.u?

They are identical numerically. Signup and view all the answers

What is the mass of a substance in grams if it contains 1 mole of atoms with an atomic mass of 12 g/mol?

12 g Signup and view all the answers

What is the molecular mass of one molecule of SO2?

64.07 amu Signup and view all the answers

How many atoms are in 2 moles of carbon?

1.21 x 10^24 atoms Signup and view all the answers

What is the meaning of Avogadro's number?

The number of particles in a mole, which equals 6.022 x 10^23 Signup and view all the answers

In the balanced equation for photosynthesis, what is the coefficient in front of H2O?

6 Signup and view all the answers

Which of the following statements about molar mass is correct?

Molar mass is the mass of one mole of any substance in grams. Signup and view all the answers

What is the mass of 0.5 mole of C, given that 1 mole of C has a mass of 12.01g?

6.005g Signup and view all the answers

What does a chemical equation represent?

The process in which substances change into new substances. Signup and view all the answers

Which of the following represents the balanced equation for the combustion of glucose?

C6H12O6 + 6O2 → 6CO2 + 6H2O Signup and view all the answers

How is molar mass expressed?

In grams per mole Signup and view all the answers

How many atoms are in one mole of a substance?

6.022 x 10^23 atoms Signup and view all the answers

Study Notes

Fundamentals of Medicinal and Pharmaceutical Chemistry

This topic covers moles, chemical equations, and reactions, specifically within the context of physiological solutions.
Recommended reading materials include "General Chemistry - The Essential Concepts" by Chang and Goldsby 7e, focusing on sections related to atomic structure, chemical formulas, atomic mass, Avogadro's number, molecular mass, chemical reactions, equations, general properties of aqueous solutions, concentration of solutions.

FUNCHEM 4 Learning Outcomes

Define key terms: molecule, molecular formula, molecular mass, mole, Avogadro's number.
Master calculations involving moles.
Demonstrate the balancing of chemical equations.
Define solutions and relate them to body systems like blood plasma, intracellular and extracellular fluids.
Apply the knowledge of solutions to medical applications.
Recall and calculate percentage (w/v%, w/w%, mg%) and molar concentrations (ppm).

What is an Atom?

An atom is the fundamental unit of an element.
Atoms combine to form chemical compounds.
Atoms comprise electrons, protons, and neutrons.
Atoms are the smallest unit capable of participating in chemical reactions.

What are Molecules?

A molecule is a collection of two or more atoms.
Molecules can be formed from the same element or different elements.
Diatomic molecules comprise two atoms.
Polyatomic molecules comprise more than two atoms.
Molecules are held together by chemical bonds.

Molecular Formula

A molecular formula precisely denotes the number of atoms of each element present in a molecule, like glucose (C₆H₁₂O₆).

Atomic Mass

Atomic mass represents the mass of an atom.
It's expressed in atomic mass units (amu) or atomic mass units (u).
Weighted average of different isotopes' atomic mass.
Carbon-12 is the reference isotope.

Molecular Mass (Molecular Weight)

Molecular mass is a sum of individual atomic masses within a molecule.
It's measured in atomic mass units (amu).
Molecular mass and molar mass are numerically equal but have distinct units.

Chemical Reactions

Chemical reactions alter substances into new ones by breaking and forming chemical bonds.
Chemical equations represent chemical reactions by using chemical symbols.
Balancing equations ensures equal atoms.

'Recipe' to make glucose

The balanced equation for glucose synthesis from carbon dioxide and water is represented as 6CO₂ + 6H₂O → C₆H₁₂O₆ + 6O₂, using sunlight.

How to measure quantities

Relating mass to the number of atoms/molecules using the mole is necessary.
Avogadro's number (6.022 x 10²³) relates moles to the number of atoms/molecules.

The Mole

The mole (mol) is a unit to count the number of particles. It's analogous to a dozen.
1 mol of any substance contains the same number of particles as 12 grams of Carbon-12.

Molar Mass

A mole of a substance will always have the molecular weight of the substance in grams/mol.
Moles is equal to mass divided by molar mass.

Balancing Chemical Equations

Proper balancing assures the same number of each atom type on both sides of a chemical equation.
A systematic method is required to ensure the correct equation is reached.

Examples

Illustrative examples demonstrate balancing equations, using appropriate coefficients.

Calculating Reactant/Product Amounts

Sequential steps for deriving necessary calculations to ascertain product or reactant amounts from balanced chemical reactions.

What is a Solution?

A solution is a homogeneous mixture of two or more elements.
Two parts make up a solution, the solute and solvent.
Solutes are present in a smaller amount and dissolved in a solvent, which is present in a greater amount.

Solution - Concentration

Concentration expresses the solute's amount in a given amount of solvent or solution.
Dilute solutions contain a small amount of solute; concentrated solutions contain a large amount of solute.

Concentration methods

Percentage concentration (w/v, w/w);
Molar concentration (molarity);
Parts per million (ppm), etc.

Intravenous Drip

IV therapy involves injecting substances directly into a vein.
Situations demanding IV solutions include patients who cannot swallow, require fast concentration of medications, poor gastrointestinal absorption.
The composition of fluids utilized in IV drips usually isotonic with blood plasma.

Example: Severe Dehydration

Injecting water directly into the body in cases of severe dehydration might cause red blood cells to swell and burst (hemolysis).
To prevent this, solutions used must be isotonic with blood plasma to avoid problems.

Milligram percent

A unit of percentage concentration, useful for expressing compounds like urea in blood.
It involves converting the amount to milligrams.

Parts per million (ppm)

ppm expresses extremely low levels of solute in a solution.
Relevant for trace elements in water or medications.

Molarity

Molarity explicitly defines the concentration of a solution.
It's determined by using the moles per litre of solution.

In Conclusion

Key concepts: physiological solutions (like 5% glucose, 0.9% saline), moles, Avogadro's number, balancing chemical equations, different concentrations (percentage and molar).
Practical applications, particularly to IV solutions and patient care, are shown.

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Description

Test your knowledge on the fundamentals of medicinal and pharmaceutical chemistry, including moles, chemical reactions, and solutions as related to physiology. This quiz is based on essential concepts from 'General Chemistry - The Essential Concepts' by Chang and Goldsby, focusing on the definition of key terms and calculations involving moles.