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:
derived unit. noun. a unit of measurement obtained by multiplication or division of the base units of a system without the introduction of numerical factors.
Explanation:
Answer:
0.595
Explanation:
Let's consider the decomposition of hydrogen chloride.
2 HCl(g) ⇄ H₂(g) + Cl₂(g)
The pressure equilibrium constant (Kp) is equal to the product of the partial pressure of the products raised to their stoichiometric coefficients divided by the product of the partial pressure of the reactants raised to their stoichiometric coefficients.
Kp = pH₂ × pCl₂ / pHCl²
Kp = 77.9 × 54.4 / 84.4²
Kp = 0.595
Assuming that the reaction is unimolecular on both
reactant and product sides such that:
HA + OH-
--> A- + H2O
Therefore the amount of A- left is:
mmol HA = 9.00 - 3.00 = 6.00 <span>
mmol A- = 3.00
pKa = - log Ka = 5.25
</span>
<span>Calculating for pH:
pH = 5.25 + log 3.00/6.00</span>
<span>
pH = 4.95 </span>
