Which of the equation below refers to the standard enthalpy of formation, ΔH f o ?

2C(s) + 2H 2 (g) ---> C 2 H 4 (g) ΔH = - 52.3 kJmol -1

Na(g) ---> Na + (g) + e - ΔH = -364 kJmol -1

C 2 H 5 OH(l) + 3O 2 (g) ---> 2CO 2 (g) + 3H 2 O (l) ΔH = - 1286 kJmol -1

When 1.0 mole of ZnO(s) decomposes, ZnO(s) ---> Zn(s) + 1/2 O 2 (g) , enthalpy change is +348 kJ/mol. What does this tell you about the formation of ZnO (s)?

the formation of ZnO (s) is exothermic

the formation of ZnO (s) is endothermic

the formation of ZnO (s) does not require energy

the formation of ZnO (s) absorbs heat.

Which statement is true regarding endothermic reactions?

c) Temperature change is negative and enthalpy change is positive

a) Temperature change is positive and enthalpy change is positive

b) Temperature change is positive and enthalpy change is negative

d) Temperature change is negative and enthalpy change is negative

d) Energy stored in the chemical bonds in a substance

a) Energy stored in the movement of molecules in a substance

c) The temperature of a molecule

Describe the energy change that takes place when bonds are broken.

c) Energy is taken in and then given out

d) Energy is given out and then taken in

Calorimetry is a technique used to

measure the enthalpy change for a reaction

Which statement is FALSE for an exothermic reaction?

Reactants have stronger bonds than products

Reactants higher in energy and less stable

Product lower in energy and more stable

Products have stronger bonds than reactants

Standard enthalpy of precipitation

What does the circle mean in ΔH°?

Standard Conditions (T=298.15 K P=1 atm)

Standard Temperature and Pressure (T=273.15 K P=1 atm)

Define the term Exothermic by picking the correct statements

Products have less energy than the reactants

Energy is given out to the surroundings (temperature goes up).

products have more energy than the reactants

Define Endothermic by picking the correct statements

products have more energy than the reactants

Energy is taken in from the surroundings (temperature goes down).

Energy is given out to the surroundings (temperature goes up).

· Products have less energy than the reactants

Which statement is true regarding endothermic reactions?

c) Temperature change is negative and enthalpy change is positive

a) Temperature change is positive and enthalpy change is positive

b) Temperature change is positive and enthalpy change is negative

d) Temperature change is negative and enthalpy change is negative

The enthalpy of neutralisation is the enthalpy change

when 1 mole of H + (aq) ions from acid reacts with 1 mole of OH - (aq) ions from an alkali to form 1 mole of water under the stated condition of the experiment

when one mole of the pure compound is formed from its elements under standard conditions

when 1 mole of pure substance is completely burned in excess oxygen, under the given temperature and pressure of the reaction

the magnitude of the enthalpy change of a chemical reaction depends only on the difference in the enthalpy content of the products and the reactants, and does not on how the reaction is completed

Which of the following equations represents the enthalpy change of combustion?

C 4 H 10 (g) +13/2O 2 (g) → 4CO 2 (g) + 5H 2 0(g)

2C 4 H 10 (g) +13O 2 (g) → 8CO 2 (g) + 10H 2 0(g)

C 4 H 10 + 9/2O 2 = 4CO (s)+ 5H 2 O

C 4 H 10 + 5/2O 2 = 4C(s) + 5H 2 O(g)

What is the standard enthalpy change of formation ?

2Fe (s) + 1 1 / 2 O 2(g) → Fe 2 O 3(s)

4Fe (s) + 3O 2 → 2 Fe 2 O 3(s)

2H 2(g) + O 2 (g) → 2H 2 O (l)

For a skillet, used for cooking, do you want a high or low specific heat

Low, so that it will change temperature quickly

High, so that it will need more energy to heat up

Calorimeters use insulating materials to:

prevent heat from escaping to the environment.

encourage affordable materials in science experiments in schools.

preserve the heat of the environment outside the Styrofoam cup.

keep the liquid inside the Styrofoam cup from overheating.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

they both have an equal temperature

one reaches a temperature of zero

Enthalpy

Quiz

•

Chemistry

•

12th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-4, HS-PS3-4, MS-PS3-3

+2

Standards-aligned

Ayunie Nadzri

Used 286+ times

FREE Resource

45 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

How do you calculate Enthalpy of a reaction?

ΔH = ΔH_products- ΔH_reactants

ΔT = q / mC

ΔG = ΔH -TΔS

E = mc²

Tags

NGSS.HS-PS1-4

2.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Specific heat capacity is

heat energy needed to raise temp by 1C

heat energy needed to raise temp of 1g of substance by 1C

heat energy absorb to raise 1g of substance to higher temp

heat energy need to raise temp for 1g of substance

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

3.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

"Heat change when 1 mole of gaseous atom is formed from its element at standard condition" is the definition for _______.

standard enthalpy of formation

standard enthalpy ofhydration

electron affinity

standard enthalpy of atomisation

4.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What is standard enthalpy of formation, ΔH_f^o?

Heat change when 1 mole of gaseous ions is hydrated in water at 25^oC and 1 atm

Heat change when 1 mole of compound is formed from its elements in their stable state at standard condition of 25^oC and 1 atm

Heat change when 1 mole of gaseous atom is formed from its elements at 25^oC and 1 atm

Heat change when 1 mole of electrons is removed from 1 mole of gaseous atoms at ground state at 25^oC and 1 atm

Tags

NGSS.HS-PS1-4

5.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Name the type of enthalpy for the following reaction:
Na⁺ (g) --> Na⁺ (aq) ΔH = -364 kJmol^-1

Standard enthalpy of neutralisation, ΔH_neut^o

Standard enthalpy of solution, ΔH_soln^o

Standard enthalpy of hydration, ΔH_hyd^o

lattice energy, ΔH_lattice^o

Tags

NGSS.HS-PS1-4

6.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Enthalpy change represented by the equation
MgSO₄ (s) ---> Mg²⁺ (aq) + SO₄ ^2- (aq)
is known as_____________.

ionization energy of magnesium and sulphate

lattice crystal energy of magnesium sulphate

enthalpy of solution of magnesium sulphate

enthalpy of hydration of magnesium sulphate

Tags

NGSS.HS-PS1-4

7.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Define standard enthalpy of combustion.

Heat released when one mole of substance is burnt completely in excess oxygen.

Heat absorbed when one mole of substance is burnt completely in excess oxygen under standard conditionj

Heat released when one mole of substance is burnt completely in excess oxygen under standard condition.

Heat change when one mole of substance is burnt partially in excess oxygen under standard condition.

Tags

NGSS.HS-PS1-4

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Enthalpy

45 questions

How do you calculate Enthalpy of a reaction?

Specific heat capacity is

"Heat change when 1 mole of gaseous atom is formed from its element at standard condition" is the definition for _______.

What is standard enthalpy of formation, ΔH_f^o?

Name the type of enthalpy for the following reaction:
Na⁺ (g) --> Na⁺ (aq) ΔH = -364 kJmol^-1

Enthalpy change represented by the equation
MgSO₄ (s) ---> Mg²⁺ (aq) + SO₄ ^2- (aq)
is known as_____________.

Define standard enthalpy of combustion.

Which of the following has a ΔH_f^o value of 0?

What is the type of standard enthalpy of this reaction?
Na(s) ---> Na(g) ΔH = +109 kJmol^-1

Which of the equation below refers to the standard enthalpy of formation, ΔH_f^o?

Create a free account and access millions of resources

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Popular Resources on Wayground

Discover more resources for Chemistry

Enthalpy

45 questions

How do you calculate Enthalpy of a reaction?

Specific heat capacity is

"Heat change when 1 mole of gaseous atom is formed from its element at standard condition" is the definition for _______.

What is standard enthalpy of formation, ΔHfo?

Name the type of enthalpy for the following reaction:Na+ (g) --> Na+ (aq) ΔH = -364 kJmol-1

Enthalpy change represented by the equation MgSO4 (s) ---> Mg2+ (aq) + SO4 2- (aq)is known as_____________.

Define standard enthalpy of combustion.

Which of the following has a ΔHfo value of 0?

What is the type of standard enthalpy of this reaction?Na(s) ---> Na(g) ΔH = +109 kJmol-1

Which of the equation below refers to the standard enthalpy of formation, ΔHfo?

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

What is standard enthalpy of formation, ΔH_f^o?

Name the type of enthalpy for the following reaction:
Na⁺ (g) --> Na⁺ (aq) ΔH = -364 kJmol^-1

Enthalpy change represented by the equation
MgSO₄ (s) ---> Mg²⁺ (aq) + SO₄ ^2- (aq)
is known as_____________.

Which of the following has a ΔH_f^o value of 0?

What is the type of standard enthalpy of this reaction?
Na(s) ---> Na(g) ΔH = +109 kJmol^-1

Which of the equation below refers to the standard enthalpy of formation, ΔH_f^o?