The elements X and Y combine in different ratios to form four different types of compounds: XY, XY2, XY3, and XY4. Consider that
there is enough of each compound to contain 2 g of X. In XY the mass of X is 2 g and the mass of Y is 4 g.
Arrange the following ratios in order of their increasing value. Rank from highest to lowest ratio. To rank items as equivalent, overlap them.
1. The ratio of the mass ratio of Y to X in XY3 to the mass ratio of Y to X in XY.
2. The ratio of the mass ratio of Y to X in XY2 to the mass ratio of Y to X in XY.
3. The ratio of the mass ratio of Y to X in XY4 to the mass ratio of Y to X in XY.
Arrange the following ratios in order of their increasing value. Rank from highest to lowest ratio. To rank items as equivalent, overlap them.
1. The ratio of the mass ratio of Y to X in XY3 to the mass ratio of Y to X in XY.
2. The ratio of the mass ratio of Y to X in XY2 to the mass ratio of Y to X in XY.
3. The ratio of the mass ratio of Y to X in XY4 to the mass ratio of Y to X in XY.
1 answer:
Answer:
Ratios in order of increasing value ; The ratio of the mass ratio of Y to X in XY2 to the mass ratio of Y to X in XY, The ratio of the mass ratio of Y to X in XY3 to the mass ratio of Y to X in XY, The ratio of the mass ratio of Y to X in XY4 to the mass ratio of Y to X in XY
1) Mass ratio = 3
2) Mass ratio = 2
3) Mass ratio = 4
Explanation:
The detailed and step by step calculation is shown in the attachment.
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The average atomic mass of the imaginary element : 47.255 amu
<h3>Further explanation </h3>The elements in nature have several types of isotopes
Isotopes are elements that have the same Atomic Number (Proton)
Atomic mass is the average atomic mass of all its isotopes
Mass atom X = mass isotope 1 . % + mass isotope 2.% ..
isotope E-47 47.011 amu, 87.34%
isotope E-48 48.008 amu, 6.895
isotope E-49 50.009 amu, 5.77%
The average atomic mass :