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2 years ago

BALANCE THIS EQUATION: C4H10 + O2 = C02 + H20

Chemistry

1 answer:

Lostsunrise [7]2 years ago

5 0

Answer:

${ \rm{C _{4} H_{10}+ \frac{13}{2} O _{2} = 4C0 _{2} + 5H _{2}0}} \\$

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PLEASE HELP ME I BEG YOU

slamgirl [31]

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3) FALSE

4) FALSE

5) FALSE(i think)

6) TRUE

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3 years ago

Read 2 more answers

The pressure on a 200 milliliter sample of CO2 (g) at constant temperature is increased from

balu736 [363]

The answer for the following problem is mentioned below.

Therefore the final volume of the gas is 100 ml.

Explanation:

Given:

Initial pressure ( $P_{1}$ ) = 600 mm of Hg

Final pressure ( $P_{2}$ ) = 1200 mm of Hg

Initial volume ( $V_{1}$ ) = 200 ml

To find:

Final volume ( $V_{2}$ )

We know;

According to the ideal gas equation,

P × V = n × R × T

Where;

P represents the pressure of the gas

V represents the volume of the gas

n represents the no of moles of the gas

R represents the universal gas constant

T represents the temperature of the gas

So,

From the above mentioned equation,

P × V = constant

$\frac{P_{1} }{P_{2} }$ = $\frac{V_{1} }{V_{2} }$

Where,

( $P_{1}$ ) represents the initial pressure of the gas

( $P_{2}$ ) represents the final pressure of the gas

( $V_{1}$ ) represents the initial volume of the gas

( $V_{2}$ ) represents the final volume of the gas

So;

$\frac{600}{1200}$ = $\frac{V_{2} }{200}$

$V_{2}$ = 100 ml

Therefore the final volume of the gas is 100 ml.

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Which of the following particles combine to form molecules?

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Answer:

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Oxidation number of J = 0

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2 years ago