An element consists of two isotopes. one with a mass of 79.95 amu and an abundance of 29.9%. the second isotope has a mass of 81.95 amu with an abundance of 70.1%. what is the molar mass of this element?

 the molar  mass of the element  is  81.36 g/mol

calculation

step 1 : multiply  each %abundance  of the isotope  by   its mass  number

that is 79.95 x 29.9 =2391

           81.95 x 70.1  = 5745

Step 2: add them together

2390.5 + 5744.7 =8136

Step 3: divide by 100

= 8136/100 = 81.36  g/mol

specific gravity is the density of a substance divided by the density of water. since (at standard temperature and pressure) water has a density of 1 gram/cm3, and since all of the units cancel, specific gravity is usually very close to the same value as density

so "c" is the answer

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in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm