The solubility of a compound with a molecular weight of 233.2 is determined to be 27.9 g in 125.0 g of water at 398 K. Express t
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<u>Answer:</u> The mass or zinc reacted is 0.624 grams.
<u>Explanation:</u>
We are given:
Total pressure = 1.032 atm
Vapor pressure of water = 32 torr = 0.042 atm (Conversion factor: 1 atm = 760 torr)
To calculate partial pressure of hydrogen gas, we use the equation:
To calculate the number of moles of hydrogen gas, we use the equation given by ideal gas follows:
where,
P = pressure of hydrogen gas = 0.99 atm
V = Volume of hydrogen gas = 240. mL = 0.240 L (Conversion factor: 1 L = 1000 mL)
T = Temperature of hydrogen gas =
R = Gas constant =
n = number of moles of hydrogen gas = ?
Putting values in above equation, we get:
The chemical equation for the reaction of zinc and hydrochloric acid follows:
By Stoichiometry of the reaction:
1 mole of hydrogen gas is produced from 1 mole of zinc metal
So, of hydrogen gas is produced from =
of zinc metal
To calculate the mass of zinc metal, we use the equation:
Molar mass of zinc = 65.38 g/mol
Moles of zinc = moles
Putting values in above equation, we get:
Hence, the mass or zinc reacted is 0.624 grams.
Answer:
Explanation:
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In this case, it is possible to propose an energy balance in order to illustrate how the heat released by the reaction is absorbed by the water:
Thus, since the heat released by the reaction is -112 kJ (-112000 J), it is possible to define the hear absorbed by the water in terms of mass, specific heat and temperature change:
In such a way, it is possible to define the final temperature as shown below:
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