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3 years ago

Write the balanced equation showing the decomposition of carbonic acid and sulfurous acid.

Chemistry

1 answer:

Travka [436]3 years ago

4 0

Explanation:

here's the answer to your question

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2- How many electrons make an energy level stable (happy) ?

VARVARA [1.3K]

Most of them need 8 electrons

8 0

3 years ago

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A balloon is inflated with helium to a volume of 45L at room temperature (298K). If the balloon is cooled to 200.K, what is the

igor_vitrenko [27]

Answer:

V₂ = 30.20 L

Explanation:

Given data:

Initial volume = 45 L

Initial temperature = 298 K

Final temperature = 200 K

Final volume = ?

Solution;

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁

V₂ = 45 L × 200 K / 298 k

V₂ = 9000 L.K / 298 K

V₂ = 30.20 L

8 0

3 years ago

How many liters of phosphine are produced when 34 L of hydrogen reacts with an excess of phosphorus under STP?

Keith_Richards [23]

Answer:

22.67 L of PH₃

Explanation:

The balanced equation is:

$P_4 (s) + 6H_2(g) \to 4PH_3(g)$

From the equation:

$34 L \times \dfrac{1 \ mol \ of H_2 }{22.4 \ L \ H_2} \times \dfrac{4 \ mol \ of \ PH_3}{6 \ mol \ H_2} \times \dfrac{22.4 \ L \ PH_3}{1 \ mol \ PH_3}$

= 22.67 L of PH₃

5 0

3 years ago

Which are signs of Chemical Change (pick all that apply)

Tema [17]

might be gas change or colour change

3 0

3 years ago

Si una masa dada de hidrógeno ocupa 40 litros a 700 grados torr. ¿Qué volumen ocupará a 1 atmósfera de presión? (dar la presión

Svetach [21]

Answer:

$V_2=36.84L$

Explanation:

Hola,

En este caso, podemos usar la ley de Boyle, la cual nos permite analizar el comportamiento volumen-presión en un gas ideal de manera inversamente propocional:

$P_1V_1=P_2V_2$

Así, dado el volumen y la presión inicial, la cual se convierte a atmósferas (760 torr = 1atm), calculamos el volumen final a 1 atm como se muestra a continuación:

$V_2=\frac{P_1V_1}{P_2}=\frac{700torr*\frac{1atm}{760torr}*40l }{1atm}\\ \\V_2=36.84L$

Saludos!

7 0

3 years ago

Read 2 more answers