Ahydrated compound has analysis of 18.29% ca, 32.37%ci, and49.34%h2o. what's its formula?

CaCl₂.6H₂O

Explanation:

No. of moles of Ca = (18.29 g) / (40.0 g/mol) = 0.457 mol.

No. of moles of Cl = (32.37 g) / (35.4 g/mol) = 0.914 mol.

No. of moles of H₂O = (49.34 g) / (18.0 g/mol) = 2.74 mol.

So the mole ratio of (Ca: Cl: H₂O) is (1: 2: 6).

So, the formula of the compound is CaCl₂.6H₂O.

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.