The final temperature : 78.925°C
<h3>Further explanation </h3>Heat can be calculated using the formula:
Q = mc∆T
Q = heat, J
m = mass, g
c = specific heat, joules / g ° C
∆T = temperature difference, ° C / K
Energy releases = 130 kcal = 130 x 4.18 kJ=543.4 kJ
The final temperature :
Final temperature :
ΔT=final-initial
51.925°c=final-27°c
final = 51.925+27=78.925°C
Answer: The moles of gas present in the cylinder is 0.34 moles.
Explanation:
Given: = 2.7 atm,
= 3.1 L,
= 300 K
= ?,
= 9.4 L,
= 610 K
Formula used to calculate the final temperature is as follows.
Substitute the values into above formula as follows.
Now, moles present upon heating the cylinder are as follows.
Thus, we can conclude that moles of gas present in the cylinder is 0.34 moles.
Answer:
The wavelength the student should use is 700 nm.
Explanation:
Attached below you can find the diagram I found for this question elsewhere.
Because the idea is to minimize the interference of the Co⁺²(aq) species, we should <u>choose a wavelength in which its absorbance is minimum</u>.
At 400 nm Co⁺²(aq) shows no absorbance, however neither does Cu⁺²(aq). While at 700 nm Co⁺²(aq) shows no absorbance and Cu⁺²(aq) does.
<u>Answer:</u> The heat required for the process is 4.24 kJ
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
Given mass of benzene = 24.8 g
Molar mass of benzene = 78.11 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 absorbed = ?
n = number of moles = 0.318 moles
= enthalpy change of the reaction = 30.7 kJ/mol
Putting values in above equation, we get:
Hence, the heat required for the process is 4.24 kJ