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1 year ago

When 2 moles of C6H6 react with excess Oxygen gas, how many moles of water are produced?

Chemistry

1 answer:

Phoenix [80]1 year ago

5 0

Answer:

12 moles H₂O

Explanation:

To find the amount of water produced, you need to use the given amount and multiply it by the mole-to-mole ratio from the equation. These numbers are the coefficients of the molecules you are converting from and to. When writing the ratio, make sure to arrange it in a way that allows for the cancellation of units.

1 C₆H₆ + 9 O₂ ----> 6 CO₂ + 6 H₂O

2 moles C₆H₆ 6 moles H₂O
--------------------- x ------------------------- = 12 moles H₂O
1 mole C₆H₆

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You have 15.42g of C2H6. How many moles of H2O can be made?

Amiraneli [1.4K]

Answer: The moles of water produced are 1.54 moles.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of ethane = 15.42 g

Molar mass of ethane = 30.07 g/mol

Putting values in above equation, we get:

$\text{Moles of ethane}=\frac{15.42g}{30.07g/mol}=0.513mol$

The chemical equation for the combustion of ethane follows:

$2C_2H_6+5O_2\rightarrow 4CO2+6H_2O$

By Stoichiometry of the reaction:

2 moles of ethane produces 6 moles of water

So, 0.513 moles of ethane will produce = $\frac{6}{2}\times 0.513=1.54mol$ of water

Hence, the moles of water produced are 1.54 moles.

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3 years ago

21,980 mg of phosphorus reacts in a gas jar containing oxygen. The resulting oxide weighed 50.000 g. The percent composition of

stealth61 [152]

Answer: False

Explanation:

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2 years ago

Which type of fermentation occurs in yeast?

otez555 [7]

Fermentation occur in yeast is alcoholic.

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2 years ago

the normal boiling point of ethanol is 78.3 and its molar heat of vaporization is 393. Calculate the vapor pressure of ethanol a

madam [21]

0.12 atm vapor pressure of ethanol at 45.0 C.

What is vapor pressure in science definition?

Vapour pressure is a measure of the tendency of a material to change into the gaseous or vapour state, and it increases with temperature.
The temperature at which the vapour pressure at the surface of a liquid becomes equal to the pressure exerted by the surroundings is called the boiling point of the liquid.

We will use the Clausius-Clapeyron equation,

ln(P2/P1) = dHvap/R[1/T1-1/T2]

where,

P1 = unknown

P2 = 1 atm

T1 = 30 oC = 30 + 273 = 303 K

T2 = 78.3 oC = 78.3 + 273 = 351.3 K

dHvap = 39.3 kJ/mol = 39300 J/mol

R = 8.314 J/K.mol

Feed values,

ln(1/P1) = 39300/8.314[1/303 - 1/351.3]

P1 = 0.12 atm

thus, the vapor pressure at 30° C is 0.12 atm.

Learn more about vapor pressure

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1 year ago

PLEASE ANWSER FAST! Gus is performing an experiment on cells. First he places the cells in a container of water and salt. When h

natta225 [31]

Answer:

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2 years ago

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