Given the following reaction: \ce{Cu + 2AgNO3 -> 2Ag + Cu(NO3)2}Cu+2AgNO3 2Ag+Cu(NOX 3 )X 2 How many moles of \ce{Ag}
2 answers:
Answer:
0.252 mol
Explanation:
<em>Given the following reaction: </em>
<em>Cu + 2 AgNO₃ → 2 Ag + Cu(NO₃)₂</em>
<em>How many moles of Ag will be produced from 16.0 g Cu, assuming AgNO3 is available in excess.</em>
First, we write the balanced equation.
Cu + 2 AgNO₃ → 2 Ag + Cu(NO₃)₂
We can establish the following relations.
- The molar mass of Cu is 63.55 g/mol.
- The molar ratio of Cu to Ag is 1:1.
The moles of Ag produced from 16.0 g of Cu are:
Answer:
Explanation:
Hello,
In this case, the undergoing chemical reaction is:
As the silver nitrate is in excess, the yielded moles of silver are computed from the 16g of copper as shown below, including the corresponding stoichiometric 1 to 2 relationship between copper and silver respectively:
Best regards.
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<u>Answer:</u> The heat capacity of calorimeter is
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
Given mass of ethanol = 21.8 g
Molar mass of ethanol = 46.07 g/mol
Putting values in above equation, we get:
To calculate the enthalpy change of the reaction, we use the equation:
where,
= amount of heat released = ?
n = number of moles = 0.473 moles
= enthalpy change of the reaction = -1235 kJ/mol =
(Conversion factor: 1 kJ = 1000 J)
Putting values in above equation, we get:
To calculate the heat capacity of calorimeter, we use the equation:
where,
q = heat absorbed by the calorimeter =
c = heat capacity = ?
= change in temperature =
Putting values in above equation, we get:
Hence, the heat capacity of calorimeter is