<u>Answer:</u>
<u>For a:</u> Work done for the given reaction is 2477.572 J.
<u>For b:</u> Work done for the given reaction is 0 J
<u>Explanation:</u>
To calculate the work done for the reaction, we use the equation:
Ideal gas equation follows:
Relating both the above equations, we get:
......(1)
where,
= difference in number of moles of products and reactants = 
R = Gas constant = 8.314 J/K.mol
T = temperature = ![25^oC=[273+25]K=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B273%2B25%5DK%3D298K)
The chemical reaction follows:
Putting values in equation 1, we get:
Hence, work done for the given reaction is 2477.572 J.
The chemical reaction follows:
Putting values in equation 1, we get:
Hence, work done for the given reaction is 0 J.
Answer:
it can help heat or cool a room.
Explanation:
I think this is right...
Answer:
The balanced equation is:
2 HNO3 + Mg ---> Mg(NO3)2 + H2
From the equation, we can see that we need twice the moles of HNO3 than the moles of Mg
Moles of Mg:
Molar mass of Mg = 24 g/mol
Moles = Given mass / Molar Mass
Moles of Mg = 4.47 / 24 = 0.18 moles (approx)
Hence, 2(moles of Mg) = 0.36 moles of HNO3 will be consumed
Number of moles of HNO3 after the reaction is finished is the number of unreacted moles of HNO3
Unreacted moles of HNO3 = Total Moles - Moles consumed
Unreacted moles of HNO3 = 0.64 moles (approx)
Since we approximated the value of moles of Mg, the value of remaining moles of HNO3 will also be approximate
From the given options, we can see that 0.632 moles is the closest value to our answer
Therefore, 0.632 moles will remain after the reaction
