= 9.1 × 10^6
(scientific notation)
= 9.1e6
(scientific e notation)
= 9.1 × 10^6
(engineering notation)
(million; prefix mega- (M))
= 9100000
<span>(real number)</span>
Answer:
%Sgr = 1% (1 sig.fig.)
Explanation:
mass water = 350ml x 0.975g/ml = 341.25g
mass sugar added = 4g
solution mass = 341.25g + 4g = 345.25g
%sugar = (4g/345.25g)·100% = 1.1586% ≅ 1% (1 sig.fig)
Answer:
Option (C) 1 × 10^−12
Explanation:
Step 1:
Data obtained from the question include:
[H+] = 1x10^−2
[OH−] =?
Step 2:
Determination of [OH−] . This is illustrated below:
[H+] x [OH−] = 1x10^-14
1x10^−2 x [OH−] = 1x10^-14
Divide both side by 1x10^−2
[OH−] = 1x10^-14 / 1x10^−2
[OH−] = 1x10^-12
Therefore, the [OH−] of the solution is 1x10^-12
Answer is: C. CH3CHOHCH3.
Balanced chemical reaction of hydration of propene:
CH₃CH=CH₂ + H₂O → CH₃CHOHCH₃.
A hydroxyl group (OH⁻) attaches to one carbon of the double bond and a proton (H⁺) adds to the other carbon of the double bond according to Markovnikov's rule (hydrogen gets attached to the carbon with more hydrogen substituents).
Product of this reaction is propan-2-ol (isopropyl alcohol).
Answer:- 6984 kJ of heat is produced.
Solution:- From given information, 1367 kJ of heat is produced by the combustion of 1 mole of ethanol. We are asked to calculate the heat produced by the combustion of 235.0 g of ethanol.
Let's convert given grams to moles and multiply by the heat produced by one mole of ethanol to get the total heat produced. Molar mass of ethanol is 46 grams per mole. The set will be:
= 6984 kJ
So, 6984 kJ of heat is produced by the combustion of 235.0 g of liquid ethanol.
