Al S
1) <u> 35.94 </u> =1.33111 <u> 64.06 </u> = 2.001875
27 32
2) = <u> 1.33111 </u> = <u> 2.001875 </u>
1.33111 1.33111
3) = ( 1 ) × 2 = ( 1.5 ) ×2
4) = 2 = 3
Empirical Formula = Al2S3
1) Divide the percentage given in question by the Relative Atomic Mass (RAM)
of the given elements.
2) When you find the answers of the first part of question, divide these once again but this time, by the lowest number you found in part 1.
3) and 4) Write down the values. If you get a decimal which is in between 0.3-0.7 (including the 0.3 and 0.7), you cannot make it a whole number by rounding of. Therefore, multiply the decimal with a whole number until you get a whole number as your answer. In this question, when you multiply 1.5 by 2, the answer is 3 which is a whole number. Multiply the other whole number by the same number as that you multiplied for 1.5. And use these numbers in part 4 to make the empirical formula which is Aluminium Sulfide (Al2S3)
Hope this helps you :)))
Please give this a brainliest
Answer:
lighting a match is the answer.
Al(NO3)3 + 3KOH -------> 3KNO3 + Al(OH)3
50 ml * .2 moles/ liter = .01 Moles of Al(NO3)3
200 ml * .1 moles/liter = .02 Moles of KOH
Since the ratio between the two reactants according to the chemical equation is 1:3, we would need .03 moles of one to fully react with .01 moles of the other. Since we don't, only 1/150 mole of the first reactant will react with the .02 moles of the second reactant. This will produce .02 moles of KNO3 as well as .01 moles of Al(OH)3
.02 moles KNO3 = .02(48 grams + 14 grams + 40 grams) = .02(102 grams) = 2.04 grams
A and d is physical, b and c is chemical
