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I am Lyosha [343]
3 years ago
11

Two compounds are tested for mass composition. Compound X contains 15.0 grams hydrogen and 120.0 grams oxygen. Compound Y contai

ns 2.0 grams of hydrogen and 32.0 grams of oxygen. Are compound X and compound Y the same compound?
Chemistry
1 answer:
4vir4ik [10]3 years ago
3 0
In order to determine if compounds X and Y are the same, the mole percentages of the elements present should be equal in both compounds.

For compound X

number of moles H = 15/ 1 =15 mol H
number of moles O = 120/ 16 = 7.5 mol O

total moles = 22.5 mol

mole percentages
% mole H = 67%
% mole O = 33%

For compound Y 

mole of H = 2 /1 = 2
mole of O = 32/16 = 2

total mole = 4 mole

mol %

% mol H = 50%
% mol O = 50%

there the two compounds are not the same.
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What is the mass sample of 0.0500 moles of zinc chloride ?
vlabodo [156]

Answer:

6.82g

0.59moles

Explanation:

1. What is the mass sample of 0.0500 moles of zinc chloride ?

Given parameters:

Number of moles ZnCl₂ = 0.05moles

Unknown:

Mass of the sample  =  ?

Solution:

To find the mass of a substance using the number of moles, it would be pertinent to understand what mole is.

A mole is a substance that contains the avogadro's number of particles.

It relates to the mass using the expression below;

                Mass of a substance  = number of moles x molar mass

Molar mass of  ZnCl₂;

        Atomic mass of Zn  = 65.4g/mol

                                   Cl = 35.5g/mol

Molar mass = 65.4 + 2(35.5)  = 136.4g/mole

Mass of a substance  = 0.05 x 136.4  = 6.82g

2. How many moles of potassium sulfide are in a 65.50g sample?

Given parameters:

Mass of K₂S  = 65.5g

Unknown:

Number of moles  = ?

Solution:

The number of moles of any substance is related to mass using the expression below;

              Number of moles  = \frac{mass}{molar mass}

Molar mass of K₂S  = 2(39) + 32  = 110g/mol

              Number of moles  = \frac{65.5}{110}   = 0.59moles

8 0
3 years ago
If 2 CH3OH + 3 O2 -> 2CO2 + 4 H2O was carried out in the laboratory and 219 g of water was produced, what would the percent y
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Answer:

Percent yield = 84.5 %

Explanation:

Given data:

Mass of methanol = 229 g

Actual yield of water = 219 g

Percent yield of water = ?

Solution:

Chemical equation:

2CH₃OH + 3O₂  →  2CO₂  + 4H₂O

Number of moles of methanol:

Number of moles = mass/ molar mass

Number of moles = 229 g/ 32 g/mol

Number of moles = 7.2 mol

Now we will compare the moles of water with methanol.

                        CH₃OH         :            H₂O

                            2               :               4

                           7.2             :           4/2×7.2 = 14.4 mol

Mass of water:

Mass = number of moles × molae mass

Mass = 14.4 mol × 18 g/mol

Mass = 259.2 g

Percent yield:

Percent yield = actual yield / theoretical yield × 100

Percent yield = 219 g / 259.2 g × 100

Percent yield = 84.5 %

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