The combustion of how many moles of ethane (C₂H6) would be required to heat 740 g of water from 25.0 °C to 98.0 °C? (Assume liquid water is formed during the combustion.) Be sure your answer has the correct number of significant digits. Note: Reference the Thermodynamic properties of pure substances and Phase change properties of pure substances table for additional information. mol ethane ☐x10 x

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The combustion of how many moles of ethane (C₂H6) would be required to heat 740 g of water from 25.0 °C to 98.0 °C? (Assume liquid water is formed during
the combustion.) Be sure your answer has the correct number of significant digits.
Note: Reference the Thermodynamic properties of pure substances and Phase change properties of pure substances table for additional information.
mol ethane
X
Transcribed Image Text:The combustion of how many moles of ethane (C₂H6) would be required to heat 740 g of water from 25.0 °C to 98.0 °C? (Assume liquid water is formed during the combustion.) Be sure your answer has the correct number of significant digits. Note: Reference the Thermodynamic properties of pure substances and Phase change properties of pure substances table for additional information. mol ethane X
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According to the question,

The mass of the water = 740 gThe initial temperature = T1 = 25.0°CThe final temperature = T2 = 98.0°C

 

Find- The moles of the ethane

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