When 55.0 grams of metal at 75.0°C is added to 100. grams of water at 15.0°C, the temperature of the water rises to 18.7°C. Assu
1 answer:
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Answer:
Explanation:
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In this case, the undergoing chemical reaction is:
In such a way, the mercury II sulfate (molar mass 296.65g/mol) is in a 1:1 molar ratio with the mercury II chloride (molar mass 271.52g/mol), for that reason the stoichiometry to find mass in grams of mercury II chloride turns out:
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Answer:
Theoretical yield = 3.51 g
Explanation:
The formula for the calculation of moles is shown below:
For :-
Mass of = 1.28 g
Molar mass of = 16.04 g/mol
The formula for the calculation of moles is shown below:
Thus,
For :-
Mass of = 10.1 g
Molar mass of = 31.998 g/mol
The formula for the calculation of moles is shown below:
Thus,
According to the given reaction:
1 mole of methane gas reacts with 2 moles of oxygen gas
0.0798 mole of methane gas reacts with 2*0.0798 moles of oxygen gas
Moles of oxygen gas = 0.1596 moles
Available moles of oxygen gas = 0.3156 moles
<u>Limiting reagent is the one which is present in small amount. Thus, is limiting reagent.
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The formation of the product is governed by the limiting reagent. So,
1 mole of methane gas on reaction produces 1 mole of carbon dioxide.
0.0798 mole of methane gas on reaction produces 0.0798 mole of carbon dioxide.
Mole of carbon dioxide = 0.0798 mole
Molar mass of carbon dioxide = 44.01 g/mol
The formula for the calculation of moles is shown below:
Thus,
Mass of = 3.51 g
<u> Theoretical yield = 3.51 g</u>