A certain element found in nature has two stable isotopes, A and B. The abundanc

Question

A certain element found in nature has two stable isotopes, A and B. The abundance of one of Isotope A, which has a mass number of 62.930, is 69.15%. The atomic weight of the element is 63.546. The mass number of of Isotope B is: 62.164 62.780 63.546 63.821 64.162 64.312 64.928 66.310 None of the above; the correct answer is Consider the following elements: Ag, As, Ga, In, Sc, sn, zn. of these elements, the two which are expected to show the greatest similarity to each other in chemical properties are and The molecular formula of a certain compound is C_12H_15O_6. The empirical formula of this molecule is An isotope of a certain element has an atomic number of 96 and a mass number of 247. It forms an ion with a charge of 3+. This ion has protons, neutrons and electrons. According to the periodic table, the most stable ion of radium (Ra) is expected to be According to the periodic table, the following compound is expected to be molecular: CS_2. Cs_3N LiBr MgCI_2 KI Na_2S RaO YF_3

Explanation / Answer

Q4.

A+B isotopes

MW of A = 62.930

Abudance = 69.15%

B = X

Abundance = 100-69.15 = 30.85 %

so..

MW avergae = 63.546

MW = MW of A * Abundance of A + +MW of B * Abundance of B

63.546 = 62.930 *69.15/100 + X*30.85 /100

solve for x

X =( 63.546 -62.930 *69.15/100 ) *100/30.85

X = 64.92675 g/mol

that is for B

choose g

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