Question

9. (2 pts) There are two naturally occurring, stable isotopes for the element Iridium. Iridium has an average mass of 192.217 u. One isotope of Iridium is Ir-193, which has a natural abundance of 62.7% and a mass of 192.963 u. Using this information, determine the mass of the other isotope?

10. (2 pts) If you have 58 grams of C5H10O5 (arabinose), how many moles of arabinose do you have? How many molecules of arabinose do you have? How many hydrogen atoms do you have?






Please I need the answers to this 2 questions ASAP and explanations.
please don't try answering if you don't know what to do​

Answer 1

The answer to your questions are

a) 190.96 gr

b) 0.387 moles

c) 2.332 x 10²³ molecules

d) 10 atoms

Step-by-step explanation:

a) 192.217 u = (192.963)(0.627) + 0.373x

0.373x = 192.217 - 120.99

0.373x = 71.23

x = 190.96 g

b) MW C5H10O5 = (12 x 5) + ((10 x 1) + (16 x 5) = 150 g

= 60 + 10 + 80

= 150 g

150 g ---------------- 1 mol

58 g ------------- x

x = 58 x 1/150 = 0.387 moles

1 mol ---------------- 6 .023 x 10²³ molecules

0.387 mol ----------- x

x = 0.387 x 6 .023 x 10²³/1 = 2.331 x 10²³ molecules

Answer 2

192.217+62.7-192.963