Mixture because your pouring something into it then stirring it i don’t know.
Answer:
Enthalpy change = 74.36 kJ
Explanation:
Enthalpy change is defines as the heat absorbed or evolved during a chemical reaction at constant pressure and volume
Reaction:
H2O(l) --> H2O(g)
DHr = mCsDT
Where m is the mass of water
Cs is the specific heat capacity
DT is the temperature difference
= 31.6 * 4.18 * (25 - 3.2)
= 2879.518 J
DHvap = 44kJ/mol
Moles of water = mass/molecular weight
Molecular weight = (1*2) + 16
= 18g/mol
Moles of water = 31.6/18
= 1.756 moles
DHvap = 44 * 1.756
= 77.244kJ
DH = DHproduct - DHreactant
DHproduct = DHvap = 77.24kJ
DHreactant = DHr = 2879.518J = 2.880kJ
= 77.24 - 2.880
DH = 74.36kJ
Enthalpy change = 74.36 kJ
Answer:
10.52g KOH
Explanation:
250.0 ml X 1L/1000ml X 0.75 mol KOH/1L X 56.105gKOH/1 mol KOH =10.52g KOH
The formula or chemical formula of a compound is same irrespective of source / mode of synthesis . Thus if a sample of compound has one carbon atom for every two atoms of oxygen (CO2), the formula will remains the same
So the answer is that for all other samples the compound X should hold this ration true.
