Free Printable T2-Mock-10 ASP

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T2-Mock-10 ASP

Total questions: 61

Worksheet time: 2hrs 34mins

Name

Class

Date

If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal? (show your work)

2.34 J/g°C

0.472 J/g°C

6.13 J/g°C

0.163 J/g°C

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?

12.82 °C

24.12 °C

351 °C

Refer the the following question:
2N₂ + 3H₂ --> 2NH₃ + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?

92 kJ

0.143 kJ

23 kJ

15 kJ

What mass of P₄ must be reacted to produce 5905 kJ of energy?
P₄ + 6Cl₂ --> 4PCl₃ + 2439 kJ

25.43 g

563.0 g

2.421 g

300.0 g

Which of the following shows the enthalpy of formation of sodium iodide

Na_(s) + 1/2 I_2(s) --> NaI_(s)

Na_(s) + 1/2 I_2(g) --> NaI_(s)

Na_(s) + I_(g)--> NaI _(s)

Na⁺_(g) + I^-_(g)--> NaI _(s)

Calculate the enthalpy of reaction (ΔH).

4CO_{2 (g)} + 6H₂O _(g) → 2C₂H_{6 (g)} + 7O_{2 (g)}

ΔH_f^o [CO_2(g)] = -393.5 kJ

ΔH_f^o[H₂O_(g)] = -241.8 kJ

ΔH_f^o [C₂H_6(g)] = -84.7 kJ

550.647 KJ/mol

2855.584 KJ/mol

-550.647 KJ/mol

-2855.584 KJ/mol

Given the following data:
ΔH^○_f[FeO(s)] = –270kJmol^–1
ΔH^○_f [Fe₂O₃(s)] = –820 kJ mol^–1Select the correct equation which gives the enthalpy change, in kJ mol^–1, for the reaction:
2FeO(s) + 1⁄2O₂(g) → Fe₂O₃(s)

(–820 × 1⁄2) + 270 = –140

(+820 × 1⁄2) – 270 = +140

–820 + (270 × 2) = –280

+820 – (270 × 2) = +280

10.

11.

12.

When methane, CH4, and oxygen, O2, are mixed in a stove and ignited, a lovely blue flame results. The balanced equation is: CH₄(g) + 2O₂(g) 2H₂O(g) + CO₂(g) What can be said about the energy involved in this chemical reaction?

I. The average kinetic energy of the products is greater than that of the reactants.

II. The chemical energy stored in the reactants is greater than the chemical energy stored in the products.

III. Chemical energy in the reactants is changed into heat energy and light energy.

I only

II only

III only

I, II, and III

13.

The combustion of titanium with oxygen produces titanium dioxide

$Ti_{\left(s\right)}+O_{2\ \left(g\right)}\ \rightarrow\ TiO_{2\ \left(s\right)}$

When 0.610 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 $\degree C$ to 50.50 $\degree C$ . In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ/mol.

2.09

4.14

-311

-0.154

$-1.98\ \times10^4$

14.

A 10.1 g sample of NaOH is dissolved in 250.0 g of water in a coffee-cup calorimeter. The temperature increases from 23.0 °C to ________°C. Specific heat of liquid water is 4.18 J/g-K and ΔH for the dissolution of sodium hydroxide in water is 44.4 kJ/mol.

35.2

24.0

33.7

33.3

40.2

15.

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 3.33 °C? (The specific heat of the solution is 3.74 J/g-K.)

-7.43

-12.51

8.20

-3.89

6.51

16.

The enthalpies of combustion of C(s), H₂(g) and C4H9OH(l) (in kJmol^-1) are as follows C(s) + O₂(g) ---> CO₂(g) ∆H=a H₂(g) + ½O₂(g) ---> H₂O(l) ∆H=b C₄H₉OH(l) + 6O₂(g) ---> 4CO₂(g) + 5H₂O(l) ∆H=c

What is the enthalpy change for the reaction shown below? 4C(g) + 5H₂(l) + ½O₂(g) ---> C₄H₉OH(l)

c – 4a – 5b

2a + 10b - c

4a + 5b - c

2a + 5b + c

17.

How much energy is required to turn 1 mole of N₂O₄(g) into 2 moles N & 4 moles O(g)?

1933 kJ

-1875 kJ

- 1933 kJ

1875 kJ

18.

Given the thermochemical equation, calculate the heat evolved when 74.6 g of sulfur dioxide (molar mass = 64.07 g/mol) is converted to sulfur dioxide.

-115 kJ

115 kJ

-115.39 kJ

115.39 kJ

19.

For which process(es) is the value of ΔH expected to be positive?

1. The temperature increases when CaCl₂ dissolves in water.

2. Steam condenses to liquid water.

3. Water boils and evaporates into steam.

4. Dry ice sublimes from solid to gas.

1 only

2 only

3 and 4

2 and 3

20.

The Equation for this reaction is:

C + O₂+ 393 kJ→ CO₂

C + O₂→ CO₂+ 393 kJ

C + O₂+ 393 kJ→ CO

C + O₂+ 110 kJ → CO

21.

Which of the following is/are TRUE about Hess' law?

I - indirect way of determining standard enthalpy of formation

II -can be applied to compounds that cannot be directly synthesized from their elements

III - the change in enthalpy is the same whether the RXN takes place in one step or in series of steps

I only

II only

III only

All of the above

22.

Calculate the total heat of the RXN in the thermochemical equatio.

-61.3 kJ

61,300 J

61.3 kJ

-61,3000 J

23.

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

#1 represents the enthalpy change for this exothermic reaction.

#2 represents the enthalpy change for this endothermic reaction.

#3 represents the enthalpy change for this endothermic reaction.

#4 represents the enthalpy change for this exothermic reaction.

24.

What is the Heat of Reaction $\Delta H$ for this reaction?

-200 KJ

200 KJ

400 KJ

-300 KJ

25.

1200 J of heat are added to a sample of gas while the gas does 400 J of work on the environment. What is the change in internal energy of the gas?

800 J

1600 J

-800 J

-1600 J

26.

4 lines

27.

4 lines

28.

4 lines

29.

4 lines

30.

4 lines

31.

4 lines

32.

4 lines

33.

Line emission spectrum shown below happens when

Electron transition from lower to higher energy level.

Electron transition from higher to lower energy level.

Electron exist in fixed energy states

Electron transition between different energy levels.

34.

Emission of light from an atom occurs when an electron

drops from a higher to a lower energy level.

jumps from a lower to a higher energy level.

moves within its atomic orbital.

falls into the nucleus.

35.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.

Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).

Lithium and cadmium are in the mixture. Strontium is not in the mixture.

Lithium and strontium are in the mixture. Cadmium is not in the mixture

Cadmium and strontium are in the mixture. Lithium is not in the mixture

All of the shown elements are present in the mixture.

36.

The unknown emissions spectra belongs to the element

Hydrogen

Mercury

Neon

Sodium

37.

What gases are in the unknown mixture?

Gas B & Gas D

Gas C & Gas B

Gas A & Gas D

Gas D & Gas C

38.

Which element(s) is/are found in the star's spectra below?

Hydrogen only

Hydrogen & Helium

Calcium only

Hydrogen & Calcium

39.

n=1 to n=2 energy level gap is shown by which line in which series of the Hydrogen spectrum?

Lyman series lowest frequency line

Balmer series lowest frequency line

Lyman series highest frequency line

Balmer series highest frequency line

Paschen series highest frequency line

40.

Which of the following statements is/are incorrect regarding the atomic emission spectrum of Hydrogen?

The radiation corresponding to the n=2 to n=1 transition has the longest wavelength in the Lyman series

The series of lines of Lyman series occurs in the ultraviolet region

Each line in the spectrum corresponds to an indefinite radiation.

Emission of radiation occurs when electrons undergo transitions from lower levels to higher energy levels.

41.

The true statements out of the following is/are:

Sunlight has a continuous spectrum

The highest frequency of the uv range is existing for the violet colour

The Lyman series formed in the Hydrogen spectrum belongs to the Infra-red region

The waves that form when the electrons are transmitted from the higher energy levels to the third energy level are belonging to the Brackett series.

42.

A radiation having a frequency of 662 nm causes the red line of Balmer series of the atomic spectrum of Hydrogen.

Select the suitable energy levels of transition to form the above relevant line on the spectrum.

n=2 to n-5

n=2 to n=3

n=3 to n=2

n=3 to n=4

n=5 to n=2

43.

The energy levels that are related with the electron transition which liberates the highest energy of the H atom is,

n=4 to n=2

n=4 to n=3

n=7 to n=5

n=6 to n=2

n=2 to n=1

44.

1. The distance between two adjacent lines in the Hydrogen spectrum increase with the increasing frequency

2. The energy gap between consecutive energy levels increase rapidly in a hydrogen atom when energy levels move further away from the nucleus.

The above 2 statements respectively are,

True , True

True , False

False , True

False , False

45.

What is the energy, in eV, of a photon that has a wavelength of 620 nm?

1eV

2eV

3eV

4eV

46.

In the photoelectric effect, if the incident photons have a wavelength that is larger than the threshold wavelength, _______.

electrons will be ejected from the metal surface

there will be photoelectric current

no electrons will be emitted from the metal surface

the kinetic energy of the ejected electrons increases

47.

A metal with a work function of 3.5 eV is exposed to photons with an energy of 3.7 eV. What is the maximum kinetic energy of the emitted photoelectrons?

0.2 eV

0.9 eV

1.1 eV

7.7 eV

48.

What is the energy of a photon with a frequency of 5x10¹⁴ Hz? (you need to do calculation. You have enough time)

2.5x10^-19 J

3.0x10^-19 J

3.3x10^-19 J

4.5x10^-19 J

49.

What is the energy of a photon with a frequency of 5x10¹⁴ Hz?

2.5x10^-19 J

3.0x10^-19 J

3.3x10^-19 J

4.5x10^-19 J

50.

If light has a wavelength of 400 nm (4x10^-9 m), what is its frequency?

8.2x10²³

7.5x10^-16

7.5x10¹⁶

7.5x10⁴

51.

4 lines

52.

4 lines

53.

4 lines

54.

Absorption of energy occurs when an electron in a lower state absorbs energy which allows the electron to enter into an excited state to jump energy levels. Identify the arrow that signifies absorption.

Yellow

Red

Green

Blue

Violet

55.

Release of energy occurs when an electron in a higher state emits energy in the form of a photon as the electron drops down from higher energy levels to lower energy levels. Identify the arrow that signifies release from the highest energy level to level 2.

Yellow

Red

Green

Blue

Violet

56.

Identify the light beam with the shortest wavelength. Hint: If velocity of the wave increases, frequency increases due to the directly proportional relationship.

v = 3 x 10¹⁸s^-1

v = 4 x 10¹⁸s^-1

v = 9 x 10¹⁸s^-1

v = 11 x 10¹⁸s^-1

57.

An electron transitions from n = 6 to n = 3. Which wavelength is released?

410 nm

1875 nm

1282 nm

1094 nm

58.

Which electron transition is associated with a higher energy wave?

n = 4 to n = 3

n = 4 to n = 2

n = 4 to n = 1

59.

Read the following statements:

I. It explains the origin of the emission spectrum for Hydrogen only.

II. It is impossible to know both the position and the momentum of the electron

III. It does not specify the position of the electron in the atom.

What options correspond to deficiencies of the Bohr's atomic model?

I and II

I and III

II and III

I, II and III

60.

When an electron moves from n=4 to n=1, what wavelength of energy is emitted?

97 nm

410 nm

434 nm

1282 nm

61.

The line with the shortest wavelength is produced in the hydrogen spectrum when electron moves

from n=2 to n=1

rom n=4 to n=1

from n=3 to n=1

from n=4 to n=3

100 %

T2-Mock-10 ASP

Total questions: 61

Worksheet time: 2hrs 34mins

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