A7.36 g sample of copper is contaminated with a additional 0.51 g sample of zinc. suppose an atomic mass measurement was performed on this sample. what would be the measured atomic mass?
64.46
63.67
63.94
65.38

The correct answer is 63.67.

Explanation:  

The atomic mass of copper is 63.546 amu

The atomic mass of zinc is 65.38 amu

The weight of total sample is 7.36 grams

Weight of zinc is 0.51 gram

Therefore, weight of copper is 7.36 - 0.51 = 6.85 grams.  

By calculating the percent composition we get:  

% of copper = 6.85 * 100 / 7.36 = 93.07 %

% of zinc = 100 - 93.07 = 6.93 %

Average atomic mass of sample = (atomic mass of copper * % copper) + (atomic mass of zinc * % of zinc) / 100

= (63.546 * 93.07) + (65.38 * 6.93) / 100

(5914.22 + 453.08) / 100

= 6367.3 / 100 = 63.67

Hence, the measured atomic mass of the sample is 63.67.  

sorry idk the answer well to you i have a explaination

explanation: a formula which shows the arrangement of atoms in the molecule of a compound

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