1. Calculate the formula mass of (NH4)3ASO4.A. 417.80 amuB. 193.05 amuC. 165.02 amuD. 156.96 amuE. 108.96 amu2. What is the mass of 1.21 × 1020 atoms of sulfur? (NA = 6.022 × 1023 mol-')XA. 3.88 × 1021 gB. 2.00 mgC. 32.06 gD. 6.44 mgE. 2.00 × 10 g3. Balance the following equation for the combustion of benzene:2 C6H6(1) + O2(g)-H2O(g) +CO2(g)->>>A. C6H6(1)+ 902(g) 3H2O(g) + 6CO2(g)B. C6H6(1)+ 902(g) →6H2O(g) + 6CO2(g)C2C6H6(1)+1502(g) → 6H2O(g) + 12CO2(g)D. C6H6(1) + 1502(g) → 3H2O(g) + 6CO2(g)E. 2C6H6(1) + 902(g) → 6H2O(g) + 12CO2(g)4. The scientist who determined the magnitude of the electric charge on the electronwasA. Robert MillikanB. J. Burdge.C. J. J. Thomson.D. Henry Moseley.E. John Dalton.5. Atoms X, Y, Z, and R have the following nuclear compositions:410-186X183410412186412,185RIIIIIIIVWhich of the following are isotopes of the same element?

1. Formula mass of a compound is the sum of the masses of all the atoms present in the compound.

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1. Calculate the formula mass of (NH4)3ASO4. A. 417.80 amu B. 193.05 amu C. 165.02 amu D. 156.96 amu E. 108.96 amu

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

1. Calculate the formula mass of (NH4)3ASO4.
A. 417.80 amu
B. 193.05 amu
C. 165.02 amu
D. 156.96 amu
E. 108.96 amu
2. What is the mass of 1.21 × 1020 atoms of sulfur? (NA = 6.022 × 1023 mol-')
X
A. 3.88 × 1021 g
B. 2.00 mg
C. 32.06 g
D. 6.44 mg
E. 2.00 × 10 g
3. Balance the following equation for the combustion of benzene:
2 C6H6(1) + O2(g)-H2O(g) +CO2(g)
->>>
A. C6H6(1)+ 902(g) 3H2O(g) + 6CO2(g)
B. C6H6(1)+ 902(g) →6H2O(g) + 6CO2(g)
C2C6H6(1)+1502(g) → 6H2O(g) + 12CO2(g)
D. C6H6(1) + 1502(g) → 3H2O(g) + 6CO2(g)
E. 2C6H6(1) + 902(g) → 6H2O(g) + 12CO2(g)
4. The scientist who determined the magnitude of the electric charge on the electron
was
A. Robert Millikan
B. J. Burdge.
C. J. J. Thomson.
D. Henry Moseley.
E. John Dalton.
5. Atoms X, Y, Z, and R have the following nuclear compositions:
410-
186X
183
410
412
186
412,
185
R
I
II
III
IV
Which of the following are isotopes of the same element?

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