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🇵🇰 UVAS DVM Admission Test · flashcards
UVAS DVM Admission Test Chemistry Flashcards
51 question-and-answer cards covering Chemistry as it is examined in UVAS DVM Admission Test. 24 of them are printed below, taken from across the deck — no signup, no paywall on the preview.
24 sample cards from the Chemistry deck
Sampled from the end of the deck, so these are different cards from the ones shown on the syllabus page.
Write the ideal gas equation and define each term.
PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant (0.0821 L·atm/mol·K), T = absolute temperature (K).
State Dalton's law of partial pressures.
The total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of the individual gases: P_total = P1 + P2 + ...
List the main types of intermolecular forces from weakest to strongest.
London dispersion forces < dipole-dipole forces < hydrogen bonding (all weaker than ionic/covalent bonds).
What is hydrogen bonding and between which atoms does it occur?
A strong dipole-dipole attraction between H bonded to a highly electronegative atom (F, O, or N) and a lone pair on F, O, or N of a neighboring molecule.
Why does water have an unusually high boiling point?
Because of extensive hydrogen bonding between water molecules, which requires extra energy to break.
What is the relationship between intermolecular forces and a liquid's vapor pressure and boiling point?
Stronger intermolecular forces give lower vapor pressure and higher boiling point; weaker forces give higher vapor pressure and lower boiling point.
Name the four main types of crystalline solids.
Ionic, covalent (network/giant), metallic, and molecular crystals.
Compare ionic and molecular crystals in terms of melting point and hardness.
Ionic crystals have high melting points and are hard but brittle; molecular crystals have low melting points and are soft due to weak intermolecular forces.
Give an example of a covalent network solid and a property it has.
Diamond (or SiO2/quartz); it is very hard with a very high melting point due to a continuous network of strong covalent bonds.
What is a reversible reaction?
A reaction in which products can react to re-form the reactants; it can proceed in both forward and backward directions, shown with a double arrow.
Define chemical equilibrium.
The state of a reversible reaction where the rates of the forward and reverse reactions are equal, so the concentrations of reactants and products remain constant.
For the reaction aA + bB <=> cC + dD, write the equilibrium constant expression Kc.
Kc = ([C]^c [D]^d) / ([A]^a [B]^b), using equilibrium molar concentrations.
What does a large Kc value (Kc >> 1) indicate about a reaction at equilibrium?
That products are favored; at equilibrium the mixture contains mostly products.
State Le Chatelier's principle.
If a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the equilibrium shifts to counteract (oppose) that change.
According to Le Chatelier's principle, how does increasing pressure affect a gaseous equilibrium?
The equilibrium shifts toward the side with fewer moles of gas to reduce the pressure.
How does increasing temperature affect an exothermic equilibrium reaction?
It shifts the equilibrium in the reverse (endothermic) direction, decreasing the yield of products and decreasing Kc.
What is Kp, and how is it related to Kc?
Kp is the equilibrium constant in terms of partial pressures of gases. Kp = Kc(RT)^(delta n), where delta n = (moles of gaseous products) - (moles of gaseous reactants).
Define the rate of a chemical reaction.
The change in concentration of a reactant or product per unit time (e.g., mol dm^-3 s^-1).
For the rate law Rate = k[A]^m[B]^n, what do m and n represent?
m and n are the orders of reaction with respect to A and B; the overall order is m + n. They are determined experimentally.
How is the order of a reaction defined?
The order is the sum of the powers to which the concentration terms are raised in the experimentally determined rate law.
List the main factors that affect the rate of a reaction.
Concentration (pressure for gases), temperature, surface area, presence of a catalyst, and the nature of the reactants.
How does a catalyst increase the rate of a reaction?
It provides an alternative reaction pathway with a lower activation energy, without being consumed in the reaction.
State the first law of thermodynamics and the equation relating internal energy, heat, and work.
Energy can neither be created nor destroyed. delta U = q + w, where delta U = change in internal energy, q = heat added to the system, w = work done on the system.
State Hess's law of constant heat summation.
The total enthalpy change of a reaction is the same whether it occurs in one step or several steps, depending only on the initial and final states (because enthalpy is a state function).
What this deck covers
The Chemistry deck follows the UVAS DVM Admission Test Chemistry syllabus — 14 chapters and 45 topics — so questions land on material that is genuinely examinable rather than trivia around it. That works out to roughly 3.6 cards per chapter.
Answers are written to be recallable, not just readable — averaging about 126 characters, which is long enough to carry the reasoning and short enough to say out loud.
A deck like this earns its keep on the second and third pass. Read the syllabus first so you know the shape of the subject, then use the cards to find the specific facts that have not stuck.
Chemistry flashcards FAQ
How many Chemistry flashcards are in this UVAS DVM Admission Test deck?
51 cards. This page previews 24 of them, sampled evenly across the deck so you can judge the difficulty before installing anything.
Are these UVAS DVM Admission Test flashcards free?
Yes. The preview here is free to read with no signup, and the full 51-card deck is free inside the Examius app.
What do the Chemistry cards cover?
They follow the UVAS DVM Admission Test Chemistry syllabus — 14 chapters and 45 topics — so the questions track what is actually examinable.
How should I use these flashcards?
Read the syllabus first so you know the shape of the subject, then drill the deck. Examius schedules each card with spaced repetition, so cards you keep missing come back sooner and ones you know drift further apart.