CxHy + O2 --> x CO2 + y/2 H2O
Find the moles of CO2 : 18.9g / 44 g/mol = .430 mol CO2 = .430 mol of C in compound
Find the moles of H2O: 5.79g / 18 g/mol = .322 mol H2O = .166 mol of H in compound
Find the mass of C and H in the compound:
.430mol x 12 = 5.16 g C
.166mol x 1g = .166g H
When you add these up they indicate a mass of 5.33 g for the compound, not 5.80g as you stated in the problem.
Therefore it is likely that either the mass of the CO2 or the mass of H20 produced is incorrect (most likely a typo).
In any event, to find the formula, you would take the moles of C and H and convert to a whole number ratio (this is usually done by dividing both of them by the smaller value).
Answer:
10.32 moles of ammonia NH₃
Explanation:
From the question given above, the following data were obtained:
Number of molecules = 6.21×10²⁴ molecules
Number of mole of NH₃ =?
The number of mole of NH₃ can be obtained as follow:
From Avogadro's hypothesis,
6.02×10²³ molecules = 1 mole
Therefore,
6.21×10²⁴ molecules = 6.21×10²⁴ / 6.02×10²³
6.21×10²⁴ molecules = 10.32 moles
Thus, 6.21×10²⁴ molecules contains 10.32 moles of ammonia NH₃
Answer is: y<span>es, because the ratios of grams and moles would be similiar.
For example, molecule of water:
1) M(H</span>₂O) = 2Ar(H) + Ar(O) · g/mol.
M(H₂O) = 2 + 16 · g/mol.
M(H₂O) = 18 g/mol; molar mass of water
Ratio grams and moles is 18 : 1.
2) if we write molar mass as ratio mole and grams (1 mol/18 g), ratio is of grams and moles is still the same 18 : 1.
Answer: B 1:2
Explanation:
i legit searched it up and the answer poped up lol