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Nataly [62]
2 years ago
10

Suppose there are two known compounds containing the generic elements X and Y. You have a 1.00-g sample of each compound. One sa

mple contains 0.25 g of X and the other contains 0.33 g of X. Identify plausible sets of formulas for these two compounds. Check all that apply.
Chemistry
1 answer:
Lapatulllka [165]2 years ago
8 0

I think the correct answers are X2Y and X3Y, X2Y5 and X3Y5, and X4Y2 and X3Y, for the following reason: 

If you look at the combining masses of X and Y in each of the two compounds, 

The first compound contains 0.25g of X combined with 0.75g of Y 
so the ratio (by mass) of X to Y = 1 : 3 

The second compound contains 0.33 g of X combined with 0.67 g of Y 
so the ratio (by mass) of X to Y = 1 : 2 

Now, you suppose to prepare each of these two compounds, starting with the same fixed mass of element Y ( I will choose 12g of Y for an easy calculation!) 

The first compound will then contain 4g of X and 12g of Y 
The second compound will then contain 6g of X and 12g of Y 

<span>The ratio which combined the masses of X and the fixed mass (12g) of Y
= 4 : 6 
<span>or 2 : 3 </span>

So, the ratio of MOLES of X which combined with the fixed amount of Y in the two compounds is also = 2 : 3 </span>

The two compounds given with the plausible formula must therefore contain the same ratio.

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Answer:

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The equation for one of the reactions in the process of turning iron ore into the metal is
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Answer:

2100g or 2.1kg

Explanation:

Based on the equation given,

One mole of Fe2O3 gives two moles of Fe

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Convert 3kg to gram

3×1000=3000grams

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3000g of Fe2O3-xg of Fe

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If 2.9g of water is heated from 23.9C to 98.9C, how much heat (in calories) was added to the water?
tensa zangetsu [6.8K]

Answer:

Explanation:

we know that

ΔH=m C ΔT

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therefore ΔH=2.9 g*4.18 j/g°C*75°C

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