How many moles of H2O are produced when 64.0 g C2H2 burns in oxygen

Answers

Answer 1

Answer: The balanced chemical reaction will be:

C2H2 + 5/2O2 = 2CO2 + H2O

We are given the amount of C2H2 being burned. This will be our starting point.

64.0 g C2H2 (1 mol C2H2 / 26.02 g C2H2) (1 mol H2O/1mol C2H2) ( 18.02 g H2O/1mol H2O) = 44.32 g H2O.

Thus, the answer is 44.32 g H2O.

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Coal and natural gas came from swamp environments, while oil came from open oceans.

B.
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Answers

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You take an ice cube (mass = 18g) from the freezer (T=-10°C) and place it on the table. Later that day, you notice a puddle of water on the table that has reached ambient room temperature (20°C). How much heat must have been absorbed to make this happen? A) 1867.0 J B) 2260.4 J C) 7897.0 J D) 42657.0 J

Answers

The amount of heat absorbed or released by the system can be determined by the equation:

U = mCpΔT
where:
m = mass of material
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A positive term means energy was absorbed.

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