Chapter 25.8, Problem 1.4ACP

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Calculate the molar mass (atomic weight) of naturally occurring uranium from the masses of the two major isotopes of uranium (235U = 235.0409; 238U = 238.0508) and their natural abundances.

Interpretation Introduction

Interpretation:

The molar mass of natural occurring uranium for the masses of the two major isotopes should be calculated

Concept introduction:

The molar mass of naturally occurring uranium is obtained from the mass of the two major isotopes of uranium–235 (235.0409) uranium–238 (238.0508) and natural abundance

99.274% of 238U and 0.720% of 235U are present in the nature.

Explanation

Naturally occurring uranium is composed of three major isotopes such as uraniumâ€“238, uraniumâ€“235, and uraniumâ€“234.

Molar mass of 238U is 238.0508â€‰g/mol

Molar mass of 235U is 235.0409â€‰g/mol

99.274% of 238U and 0.720% of 235U are present in the nature.

Hence the molar mass of uranium is expressed as

Molarâ€‰massâ€‰=â€‰M

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