Write the equation for the reaction described: A solid metal oxide, Ag2O, and hydrogen are the products of the reaction between
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Answer : The final temperature of the water is,
Explanation : Given,
Mass of benzene = 8.600 g
Molar mass of benzene = 78 g/mole
First we have to calculate the moles of benzene.
Now we have to calculate the energy of combustion.
The given balanced chemical reaction is:
According to reaction,
As, 2 moles of benzene gives 6542 kJ of energy on combustion.
So, 0.1103 mole of benzene gives of energy on combustion.
Now we have to calculate the final temperature of the water.
Formula used :
where,
= heat released = 360.7913 kJ = 36079.13 J
= mass of water = 5691 g
= specific heat of water=
= final temperature = ?
= initial temperature =
Now put all the given values in the above formula, we get:
Therefore, the final temperature of the water is,
A) 10.0g of Iron is 
of Iron.
One mole of dihydrogen is required to form one mole of iron, hence you'll need
of dihydrogen.
B) Likewise : 2.50g of Iron is
of Iron, hence we'll need 
of Fe2O3.
One mole of dihydrogen is required to form one mole of iron, hence you'll need
B) Likewise : 2.50g of Iron is