When the experiment was carried out, the temperature was 22 oC and atmospheric pressure was 1.007 atm. Using the Ideal Gas Law a
1 answer:
Answer:
number of moles of =4.16mol
Explanation:
experiment data:
temperature= =273+22 k=295k
pressure=1.007 atm
volume is missing so assuming volume-=100L
using ideal law relationship
ideal gas means gas which occupies negligible space and there is no interaction between the molecules of gases.
PV=nRT
put all the experimental data, we get
n=4.15 mol
number of moles of =4.16mol
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Answer:- .
Solution:- Mass of Iron added to water is 93.3 g. Initial temperature of iron metal is 65.58 degree C and final temperature of the system is 19.68 degree C.
temperature change, for iron metal = 65.58 - 19.68 = 45.9 degree C
specific heat for the metal is given as 0.444 J per g per degree C.
let's calculate the heat lost by iron metal using the equation:
where, q is the heat energy, m is mass, c is specific heat and delta T is change in temperature. let's plug in the values and calculate q for iron metal:
q = 1901.42 J
Using same equation we will calculate the heat gained by water.
mass of water is 75.0 g.
for water = 19.68 - 16.95 = 2.73 degree C
specific heat for water is 4.184 J pr g per degree C. Let's plug in the values:
q = 856.674 J
Total heat lost by iron metal is the sum of heat gained by water and calorimeter.
So, heat gained by calorimeter = heat lost by iron metal - geat gained by water
heat gained by calorimeter = 1901.42 J - 856.674 J = 1044.746 J
Change in temperature for calrimeter is same as for water that is 2.73 degree C
For calorimeter,
So, the heat capacity of calorimeter is .