Answer:
<h2>The answer is 14.29 %</h2>
Explanation:
The percentage error of a certain measurement can be found by using the formula
From the question
actual density = 0.70 g/mL
error = 0.8 - 0.7 = 0.1
So we have
We have the final answer as
<h3>14.29 %</h3>
Hope this helps you
Answer:
78.2°C
Explanation:
take away by the illuminus of the civilization so the radiation can oxidize the whole number of its element
Cyclohex<u>ene</u> is a cyclic, six-membered hydrocarbon that contains one double bond. The types of reactions that can occur in cyclohexene would be those that are typical with alkenes generally.
The pi-bonded electrons in the double bond are nucleophilic. So, electrophilic addition reactions could occur with cyclohexene. For example,
cyclohexene + HBr → bromocyclohexane
cyclohexene + H2O/H+ → cyclohexanol
cyclohexene + Br2 → <em>trans-</em>1,2-dibromocyclohexane (racemic)
The latter is a common test for alkenes where one adds bromine to a sample to see if there is decolorization, which would indicate the presence of nucleophilic pi bonds. Bromine, which is dark reddish-brown, will become clear as it reacts with an alkene to form a colorless haloalkane.
Cyclohexene can also be converted to the fully saturated cyclohexane by hydrogenation: cyclohexene + H2/Pd → cyclohexane.
HClO4 +NaOH -----> NaClO4 + H2O
moles of NaOH = (0.0832 x 50 ) /1000= 4.16 x10^-3 moles
since the mole ratio of HClO4 to NaOH is 1:1 the moles of HClO4 is also 4.16 x 10^-3 moles
volume of HClO4 is therefore = moles/ molarity
that is 4.16 x 10^-3mol/ 0.167 mol/L= 0.0249L
multiply by 1000 to convert to ml
0.0249 x 1000= 24.9 ml
Answer:
1.5 moles of CO₂ are produced
Explanation:
Based on the chemical equation:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O<em> -The reaction of the question is wrong-</em>
5 moles of oxygen reacts per mole of propane, C₃H₈, to produce 3 moles of CO₂ and 4 moles of water.
If 2.5 moles of oxygen react and, 5 moles of oxygen produce 3 moles of CO₂, moles of CO₂ produced are:
2.5 moles O₂ * (3 moles CO₂ / 5 moles O₂) =
<h3>1.5 moles of CO₂ are produced</h3>
