Answer:
HgO (empirical formula)
Explanation:
4.08 - 3.78 = 0.3g (oxygen)
0.02 : 0.02
0.02/0.02 : 0.02/0.02
1 : 1 (ratio)
HgO ( empirical formula)
2HgO ----> 2Hg + O2 ( your equation correct)
A beaker of water has a volume of 125mL and a density of 1.0g/mL. Calculate the mass of the water.
1 answer:
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Answer:
8740 joules are required to convert 20 grams of ice to liquid water.
Explanation:
The amount of heat required (), measured in joules, to convert ice at -50.0 ºC to liquid water at 0.0 ºC is the sum of sensible heat associated with ice and latent heat of fussion. That is:
(1)
Where:
- Mass, measured in grams.
- Specific heat of ice, measured in joules per gram-degree Celsius.
,
- Temperature, measured in degrees Celsius.
- Latent heat of fussion, measured in joules per gram.
If we know that ,
,
,
and
, then the amount of heat is:
8740 joules are required to convert 20 grams of ice to liquid water.
Answer:- Heat lost by the metal is 279.45 cal.
Solution:- This type of problems are solved by using the concept, heat given = - heat taken
Metal temperature is decreasing from 45.00 degree C to 11.08 degree C. It means the heat is lost by the metal and this heat lost by metal is gained by water and the calorimeter to raise their temperature.
the equation we use is, .
where, q is the heat energy, m is mass, c is specific heat and is change in temperature.
Combined mass of calorimeter and water is 250.0 g and the specific heat is .
for calorimeter and water (combined) = 11.08 - 10.00 = 1.08 degree C
for metal = 11.08 - 45.00 = -33.92 degree C
let's plug in the values in the above equation and calculate heat gained by combined system.
q=250.0g*\frac{1.035cal}{g.^0C}*1.08^0C
q = 279.45 cal
So, the heat lost by the metal is 279.45 cal.