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WorksheetsCET: Chemistry
Total questions: 25
Worksheet time: 23mins
Name
Class
Date
1.
Hydrocarbons are compounds composed of bonded hydrogen and carbon. They can be categorized depending on the bonds that they make. Alkynes are __________.
a)
A. Hydrocarbons that contain only single bonds.
b)
B. Hydrocarbon that contains at least one carbon-to-carbon double bond.
c)
C. Hydrocarbon that does not have any carbon bonds.
d)
D. Hydrocarbon with at least one carbon-to-carbon triple bond
2.
Which of the following is NOT a chemical reaction?
a)
A. freezing carbon dioxide
b)
B. rusting of metal
c)
C. ripening of fruit
d)
D. burning paper
3.
What are the products of the reaction of MgCl2 and KOH?
a)
A. Mg(OH)2 + KCl
b)
B. MgK + HCl
c)
C. Mg + KCl2 + H2O
d)
D. MgO + K + HCl
4.
What kind of chemical reaction is the following? CaCO3 → CaO + CO2
a)
A. Single Replacement
b)
B. Decomposition
c)
C. Double Replacement
d)
D. Combination
5.
During an experiment, Julie mixed water with Ammonium nitrate in a beaker. Upon touching the container she felt that it was cold. Why?
a)
A. An endothermic reaction occurred
b)
B. Nuclear fission just occurred
c)
C. An exothermic reaction occurred
d)
D. Nuclear fusion just occurred
6.
An element has 19 protons, 19 electrons and 24 neutrons. Find its mass number.
a)
A. 32
b)
B. 38
c)
C. 62
d)
D. 43
7.
The pH level of water is Brgy. Compostella is at 6.5. Which means that it is _____________.
a)
A. acidic
b)
D. organic
c)
C. basic
d)
D. dirty
8.
In a reaction, when the rate forward reaction is the same with the rate of the reverse reaction means ___________.
a)
A. No heat is being supplied to the reaction
b)
B. That no reaction occurred
c)
C. The concentration of the reactants is saturated
d)
D. Chemical equilibrium has been attained
9.
The medicine Paracetamol is made up of 63.58% Carbon, 5.96% Hydrogen, 9.27% Nitrogen and 21.19 % Oxygen. Using the atomic masses of the following elements, find the empirical formula of paracetamol.
C = 12.00, H = 1.00, N = 14.00, O = 16.00
C = 12.00, H = 1.00, N = 14.00, O = 16.00
a)
A. C8HN9O2
b)
B. C12HN2O4
c)
C. C8H9NO2
d)
D. C8H9N3O2
10.
Copper plating is done using copper(II) sulfate (CuSO4) which is derived from sulfuric acid (H2SO4) and CuO (copper oxide). The reaction is shown in the chemical equation below. How many grams of CuSO4 will be produced by 0.5 moles of sulfuric acid (H2SO4)?
CuO+H2SO4 → CuSO4+H2O
Molar mass of Elements
H = 1.00, O = 16.00, S= 32.07, Cu = 63.55
CuO+H2SO4 → CuSO4+H2O
Molar mass of Elements
H = 1.00, O = 16.00, S= 32.07, Cu = 63.55
a)
A. 159.62
b)
B. 48.00
c)
C. 79.81
d)
D. 63.55
11.
What is the correct balanced equation for the reaction below:
C6H14O4 + O2 → CO2 + H2O
C6H14O4 + O2 → CO2 + H2O
a)
A. 2C6H14O4 + 15/2 O2 → 6CO2 + 7H2O
b)
B. C6H14O4 + 15O2 → 6CO2 + 7H2O
c)
C. C6H14O4 + 15O2 → 12CO2 + 14H2O
d)
D. 2C6H14O4 + 15 O2 → 12CO2 + 14H2O
12.
A sample of Helium has a volume of 1000 ml at STP. Given that the Gas constant is 0.0821 L⋅atm/mol⋅K, find how many moles of helium is in the sample.
a)
A. 0.045 moles
b)
B. 45 moles
c)
C. 0.45 moles
d)
D. 4.5 moles
13.
When temperature increases, the kinetic energy of a molecules ___________.
a)
A. Increases
b)
B. Is equal with its potential energy
c)
C. Stays the same
d)
D. Decreases
14.
Atoms of the same elements having the same atomic number can have different mass number due to differences in their number of neutrons. These atoms are _______.
a)
A. Isotopes
b)
B. Protons
c)
C. Neutrons
d)
D. Isomers
15.
Two solid were placed beside each other, if one solid is hotter that the other what will happen?
a)
A. The coldness of the other solid will flow to the hotter solid.
b)
B. Both solids will maintain their temperature.
c)
C. Heat will transfer from the hotter solid to the cooler one.
d)
D. None of the above.
16.
Which of the following pairs are almost equal in mass?
a)
A. Proton and an Electron
b)
B. Proton and a Neutron
c)
C. Neutron and an Electron
d)
D. Proton and an Electron
17.
In a compound, the sum of the total positive oxidation numbers and negative oxidation numbers must be equal to -
a)
A. 0.
b)
B. 1.
c)
C. 2.
d)
D. 3.
18.
Nitrogen gas reacts with hydrogen gas to produce ammonia as shown in the following equation:
N2 + 3H2 → 2NH3
Given 7.5 mol H2, how many grams of NH3 will be produced?
atomic masses (N = 14, H = 1)
N2 + 3H2 → 2NH3
Given 7.5 mol H2, how many grams of NH3 will be produced?
atomic masses (N = 14, H = 1)
a)
A. 15 g
b)
B. 45 g
c)
C. 85 g
d)
D. 100 g
19.
A gas measures 450 mL at a temp of 30 0C, what will be its volume at 50 0C?
a)
A. (450 mL x 323 k)/303 k
b)
B. (450 mL x 303 k)/323 k
c)
C. (300 mL x 323 k)/303 k
d)
D. (303 mL x 323 k)/303 k
20.
Which of the following is NOT a noble gas?
a)
A. Kryton
b)
B. Radon
c)
C. Xenon
d)
D. Oxygen
21.
Which of the following elements can exist as mono-atomic gases in Standard Temperature and Pressure?
a)
A. Hydrogen
b)
B. Nitrogen
c)
C. Krypton
d)
D. Oxygen
22.
An atom of the isotope chlorine-37 consists of how many protons, neutrons, and electrons? (p = proton, n = neutron, e = electron)
Atomic number of chlorine is 17
Atomic number of chlorine is 17
a)
A. 17 p, 18 n, 17 e
b)
B. 17 p, 20 n, 7 e
c)
C. 17 p, 20 n, 17 e
d)
D. 17 p, 37 n, 17 e
23.
Given the following electron configuration, determine the group number and period number of the element. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
a)
A. Period 5, Group 4
b)
B. Period 4, Group 7
c)
C. Period 4, Group 5
d)
D. Period 7, Group 3
24.
Which of the elements listed below has the greatest atomic radius?
a)
A. B
b)
B. Al
c)
C. S
d)
D. P
25.
Gas A has a volume of 710.0 ml at exerted pressure of 650.0 Torr. How much space will the gas occupy at 760.0 Torr?
a)
A. 603.7 ml
b)
B. 623.7 ml
c)
C. 607.2 ml
d)
D. 602.7 ml
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