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2 years ago

6

For below checmical equation (which may or may not be balanced), list the number of each type of atom on each side of the equati

on, and determine if the equation is balanced.
2 C6H14(l) + 19 O2(g) -------> 12 CO2(g) + 14 H2O(g)

1 answer:

Olegator [25]2 years ago

5 0

Answer:

Left hand side:-

Carbon - 12

HYdrogen - 28

Oxygen - 38

Right hand side:-

Carbon - 12

Hydrogen - 28

Oxygen - 38

Since, the number of atoms each side are equal, the reaction is balanced.

Explanation:

The given reaction is:-

$2C_6H_{14}_{(l)}+19O_2_{(g)}\rightarrow 12CO_2_{(g)}+14H_2O_{(g)}$

Left hand side:-

Carbon - 12

HYdrogen - 28

Oxygen - 38

Right hand side:-

Carbon - 12

Hydrogen - 28

Oxygen - 38

<u>Since, the number of atoms each side are equal, the reaction is balanced.</u>

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3 years ago

A rigid tank that contains 2 kg of N2 at 25°C and 550 kPa is connected to another rigid tank that contains 4 kg of O2 at 25°C an

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Answer:

The volume in the first tank = 0.32 $m^{3}$

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Explanation:

<u>First Tank </u>

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<u>Second tank</u>

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This is the iso thermal mixing. i.e.

$P_{3} V_{3} = P_{1} V_{1} + P_{2} V_{2}$ ----- (1)

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3 years ago

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3 years ago

How many grams of octane (C8H18) must be burned to produce 300.0g of CO2?

nika2105 [10]

Answer:

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Explanation:

Hello there!

In this case, according to the given combustion reaction of octane, it is possible for us to perform the stoichiometric method in order to calculate the mass of octane that is required to consume 300.0 g of oxygen by considering the 2:25 mole ratio, and the molar masses of 114.22 g/mol and 32.00 g/mol respectively:

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Regards!

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2 years ago