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saveliy_v [14]
3 years ago
11

The specific heat of water is 4.184 J/g˚C How much heat energy is absorbed when 88.0 g of water is heated from 5.8 C to 35 C? (H

int: it is just like example#1). Don't forget units and round your answer to the second decimal place. *
Chemistry
1 answer:
konstantin123 [22]3 years ago
6 0

Answer:

The heat absorbed is hence 10.751.21 J

Explanation:

The heat absorbed when 88g of water is heated from 5.8°C to 35 °C is;

Heat = m c ΔT

m = 88.0 g

c = specific heat of water = 4.184 J/g°C

ΔT = ( change in temperature) = ( 35 - 5.8)°C = 29.2°C

Equating these values into the formula, we obtain;

Heat = 88* 4.184 * 29.2

Heat = 10 751.2064 J

Heat = 10 751.21 J (2 d.p)

The heat absorbed is hence 10.751.21 J

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A sample of 1.000 g of a compound containing carbon and hydrogen reacts with oxygen at elevated temperature to yield 0.692 g H₂O
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Answer :

(a) 1.000 g of compound containing carbon and hydrogen is, 0.922 g and 0.0769 g respectively.

(b) There is no other element present in the compound.

Explanation :

(a) Now we have to determine the masses of C and H in the sample.

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

C_xH_y+O_2\rightarrow CO_2+H_2O

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We are given:

Mass of CO_2=3.381g

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Molar mass of carbon dioxide = 44 g/mol

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For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 3.381 g of carbon dioxide, \frac{12}{44}\times 3.381=0.922g of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 0.692 g of water, \frac{2}{18}\times 0.692=0.0769g of hydrogen will be contained.

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(b) Now we have to determine the compound contain any other elements or not.

Mass carbon + Mass of hydrogen = 0.922 g + 0.0769 g = 0.999 g ≈ 1 g

This means that there is no other element present in the compound.

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