Give 4 Economics activities associated with water
1 answer:
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Answer:
Mass of H₂O is 3.0g
Explanation:
The reaction equation is given as:
6CO₂ + 6H₂O → C₆H₁₂O₆ + 6O₂
Parameters that are known:
Mass of CO₂ used = 7.3g
Unknown: mass of water consumed = ?
Solution
To solve this kind of problem, we simply apply some mole concept relationships.
- First, we work from the known to the unknown. From the problem, we have 7.3g of CO₂ that was used. We can find the number of moles from this value using the expression below:
Number of moles of CO₂ =
- From this number of moles of CO₂, we can use the balanced equation to relate the number of moles of CO₂ to that of H₂O:
6 moles of CO₂ reacted with 6 moles of H₂O(1:1)
- We can then use the mole relationship with mass to find the unknown.
Workings
>>>> Number of moles of CO₂ =?
Molar mass of CO₂ :
Atomic mass of C = 12g
Atomic mass of O = 16g
Molar mass of CO₂ = 12 + (2 x16) = 44gmol⁻¹
Number of moles of CO₂ = = 0.166moles
>>>>>> if 6 moles of CO₂ reacted with 6 moles of H₂O, then 0.166moles of CO₂ would produce 0.166moles of H₂O
>>>>>> Mass of water consumed = number of mole of H₂O x molar mass
Mass of H₂0 = 0.166 x ?
Molar mass of H₂O:
Atomic mass of H = 1g
Atomic mass of O = 16
Molar mass of H₂O = (2x1) + 16 = 18gmol⁻¹
Mass of H₂O = 0.166 x 18 = 3.0g
<u>Answer:</u> The enthalpy change of the reaction is -243 J/mol
<u>Explanation:</u>
The heat released by the reaction is absorbed by the calorimeter and the solution.
The chemical equation used to calculate the heat released follows:
where,
c = heat capacity of calorimeter = 1620 J/K
= change in temperature =
(Change remains same)
Putting values in above equation, we get:
<u>Sign convention of heat:</u>
When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.
For the given chemical reaction:
We are given:
Moles of monoclinic sulfur = 1 mole
- To calculate the enthalpy change of the reaction, we use the equation:
where,
q = amount of heat released = -243 J
n = number of moles = 1 mole
= enthalpy change of the reaction
Putting values in above equation, we get:
Hence, the enthalpy change of the reaction is -243 J/mol