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tino4ka555 [31]
3 years ago
9

If a gas has a volume of 750 mL at 25°c, what would the volume of the gas be at 55°c?

Chemistry
2 answers:
Airida [17]3 years ago
4 0

825.5mL

To find this, use the equation \frac{V1}{T1} = \frac{V2}{T2}

Make sure to convert all temperatures in Celsius to Kelvin by adding 273. Once you do that, multiply and divide accordingly to get the final answer of 825.5mL

Hope this helps!

Alex3 years ago
3 0

Answer : The final volume of gas will be, 681.4 ml

Explanation :

Charles' Law : This law states that volume of gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

V\propto T     (At constant pressure and number of moles)

or,

\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1 = initial volume of gas = 750 ml

V_2 = final volume of gas = ?

T_1 = initial temperature of gas = 25^oC=273+25=298K

T_2 = final temperature of gas = 55^oC=273+55=328K

Now put all the given values in the above formula, we get the final volume of gas.

\frac{750ml}{298K}=\frac{V_2}{328K}

V_2=681.4ml

Therefore, the final volume of gas will be, 681.4 ml

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Find the volume of hydrogen gas formed when 1.5g of aluminum reacts with aq NaOH at 27 degrees Celcius.
Rudiy27

Answer:

how can I solve this ?4Al+3O2 produce 2Al2O3 find a) oxygen atoms needed to react with 5.4 g of aluminium b) grams of oxygen needed to react with 0.6 mol of aluminium?

(A) n=m/M,

n(Al)=5.4/27=0.2 moles

n(O2)=n(Al)*3/4=0.2*3/4=0.15 moles

Number of oxygen atoms= n(O2)*Avogadro's number

=0.15*6.02*10^23=9.03*10^22 oxgyen atoms

(B)

n=m/M

n(Al)=0.6/27=0.02222 moles

n(O2)=n(Al)*3/4=0.016666 moles

m=n*M

m(O2)=0.0166666*32=0.53333 grams

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2 years ago
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<h2>168 N</h2>

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The force acting on an object given it's mass and acceleration can be found by using the formula

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From the question we have

force = 56 × 3

We have the final answer as

<h3>168 N</h3>

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Hope it helped :)

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