Asample of ethanol (c2h6o) has a mass of 0.2301 g. complete combustion of this sample causes the temperature of a bomb calorimeter to increase by 1.33°c. the calorimeter has a mass of 2.000 kg and a specific heat of 2.45 j/g•°c. how many moles of ethanol are present in the sample?

   moles

Explanation:

According to avogadro's law, 1 mole of every substance weighs equal to molecular mass , occupies 22.4 L at STP and contains avogadro's number of particles.

To calculate the moles, we use the equation:

Given mass of ethanol = 0.2301

Molar mass of ethanol = 46.07 g/mol

Thus there are  moles of ethanol are present in the sample.

the answer is 6.52 for the first one then the second one is 0.004993 and finally, 1,310

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it is a solid

explanation:

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.