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sladkih [1.3K]
3 years ago
9

In 1928, 47.5 g of a new element was isolated from 660 kg of the ore molybdenite. the percent by mass of this element in the ore

was:
Chemistry
2 answers:
vitfil [10]3 years ago
8 0

To take the percent by mass of this element, we use the formula:

% mass = (mass of element / mass of ore) * 100%

% mass = (47.5 g / (660 kg * 1000 g / kg)) * 100*

<span>% mass = 7.20 x 10^-3 %</span>

patriot [66]3 years ago
3 0

<u>Answer:</u> The mass percent of element in the ore is 0.0072 %

<u>Explanation:</u>

To calculate the mass percentage of element in ore, we use the equation:

\text{Mass percent of element}=\frac{\text{Mass of element}}{\text{Mass of ore}}\times 100

Mass of element = 47.5 g

Mass of ore = 660 kg = 660000 g    (Conversion factor:  1 kg = 1000 g)

Putting values in above equation, we get:

\text{Mass percent of element}=\frac{47.5g}{660000g}\times 100=0.0072\%

Hence, the mass percent of element in the ore is 0.0072 %

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What was the purpose of putting distilled water in the blank cuvette? if your unknown used ethanol as the base solvent, what wou
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If the unknown being determined is prepared using ethanol as the base solution, the blank used must be ethanol. This is because absorbance if any from the solvent, ethanol must be zeroed out as when the measurement of the actual unknown is being made, the absorbance of the solvent does not interfere.

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Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation:
rusak2 [61]

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60.42% is the percent yield of the reaction.

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Moles of water vapors at 700 Torr and a temperature of 125 °C.

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CH_4(g)+H_2O(g)\rightarrow CO(g)+3H_2(g)

According to reaction , 1 mol of methane reacts with 1 mol of water vapor. As we can see that moles of water vapors are in lessor amount which means it is a limiting reagent and formation of hydrogen gas will depend upon moles of water vapors.

According to reaction 1 mol of water vapor gives 3 moles of hydrogen gas.

Then 0.6402 moles of water vapor will give:

\frac{3}{1}\times 0.6402 mol=1.9208 mol of hydrogen gas

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The reaction produces 26.0 L of hydrogen gas measured at STP.

At STP, 1 mole of gas occupies 22.4 L of volume.

Then 26 L of volume of gas will be occupied by:

\frac{1}{22.4 L}\times 26 L= 1.1607 mol

Moles of hydrogen gas obtained experimentally = 1.1607 mol

Percentage yield of hydrogen gas of the reaction:

\frac{Experimental}{Theoretical}\times 100

\%=\frac{ 1.1607 mol}{1.9208 mol}\times 100=60.42\%

60.42% is the percent yield of the reaction.

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