The molecular formula of the compound is C12H15O3 hence the molar mass of the compound is 207 g/mol.
We need to obtain the number of moles of carbon, hydrogen and oxygen in the compound;
Carbon = 24.91 g/44g/mol × 1 mole of carbon = 0.566 moles
Mass of carbon = 0.566 moles × 12 g/mol = 6.792 g
Number of moles of hydrogen = 6.522 g/18 g/mol × 2 moles = 0.725 moles
Mass of hydrogen = 0.725 moles × 1 g/mol = 0.725 g
Mass of oxygen = 10 - (6.792 g + 0.725 g) = 2.483 g
Number of moles of oxygen = 2.483 g/16 g/mol = 0.155 moles
Now we must divide through by the lowest number of moles;
C - 0.566/0.155 H - 0.725/0.155 O - 0.155/0.155
C - 4 H - 5 O - 1
The simplest formula is C4H5O Recall that the molar mass of the compound lies between 150.0 and 220.0 g/mol
4(12) + 5(1) + 16 = 69
Hence; n = 3 and the molecular formula of the compound is C12H15O3
The molar mass of the compound is; 12(12) + 15(1) + 3(16) = 207 g/mol
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Answer:
Endothermic
It absorbs heat
1.20 × 10³ kJ
Explanation:
Let's consider the following thermochemical equation.
2 H₂O(l) → 2 H₂(g) + O₂(g) ΔH = 572 kJ
Since ΔH > 0, the reaction is endothermic, that is, it absorbs heat when H₂O reacts.
572 kJ are absorbed when 36.03 g of water react. The heat absorbed when 75.8 g of H₂O react is:
75.8 g H₂O × (572 kJ/36.03 g H₂O) = 1.20 × 10³ kJ
The volume of the dry gas at stp is calculated as follows
calculate the number on moles by use of PV =nRT where n is the number of moles
n is therefore = Pv/RT
P = 0.930 atm
R(gas contant= 0.0821 L.atm/k.mol
V= 93ml to liters = 93/1000= 0.093L
T= 10 + 273.15 = 283.15k
n= (0.930 x0.093) /(0.0821 x283.15) = 3. 72 x10^-3 moles
At STp 1 mole = 22.4L
what about 3.72 x10^-3 moles
by cross multiplication
volume = (3.72 x10^-3)mole x 22.4L/ 1 moles = 0.083 L or 83.3 Ml
Answer:
Option c. Neutral
Explanation:
Only neutral solution gives a green colouration to a pH paper
