Answer:
Explanation:
Given data:
Mass of mixture = 454 kg
Initial temperature is 10°C
Heat added is Q = 121300 kJ
Heat capacity (Applesuace) at 32.8°C is 4.02kJ/kg K
From heat equation we have
Putting all value to get required final temperature value
<u>Answer:</u> The volume of hydrogen gas collected over water is 2.13 L
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
Given mass of zinc = 5.566 g
Molar mass of zinc = 65.4 g/mol
Putting values in above equation, we get:
For the given chemical reaction:
As, HCl is present in excess. So, it is considered as an excess reagent.
Zinc is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of zinc produces 1 mole of hydrogen gas.
So, 0.0851 moles of zinc will produce = of hydrogen gas
To calculate the volume of hydrogen gas, we use ideal gas equation, which is:
PV = nRT
where,
P = Pressure of hydrogen gas = Total atmospheric pressure - vapor pressure of water = (752 - 18.65) mmHg = 733.35 mmHg
V = Volume of the hydrogen gas
n = number of moles of gas = 0.0851 moles
R = Gas constant =
T = Temperature of hydrogen gas =
Putting values in above equation, we get:
Hence, the volume of hydrogen gas collected over water is 2.13 L
Answer : The mass of water produced will be 32.78 grams.
Explanation : Given,
Mass of = 21.9 g
Molar mass of = 72.15 g/mole
Molar mass of = 18 g/mole
First we have to calculate the moles of .
Now we have to calculate the moles of .
The balanced chemical reaction will be,
From the balanced reaction we conclude that
As, 1 mole of react to give 6 moles of
So, 0.3035 moles of react to give
moles of
Now we have to calculate the mass of .
Therefore, the mass of water produced will be 32.78 grams.