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irinina [24]
2 years ago
8

Which type of stoichiometry problems does not require the use of molar mass?

Chemistry
1 answer:
Arlecino [84]2 years ago
7 0

Answer:

Explanation:

It is volume-volume problems that does not require the use of molar mass.

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Calcular la presión final de un gas que inicialmente está a 21°C y 0,98 atm. Sabiendo que su temperatura aumenta a 37°C.
KatRina [158]

Answer:

1.03 atm

Explanation:

Primero <u>convertimos 21 °C y 37 °C a K</u>:

  • 21 °C + 273.16 = 294.16 K
  • 37 °C + 273.16 = 310.16 K

Una vez tenemos las temperaturas absolutas, podemos resolver este problema usando la<em> ley de Gay-Lussac</em>:

  • T₁P₂ = T₂P₁

En este caso:

  • T₁ = 294.16 K
  • P₂ = ?
  • T₂ = 310.16 K
  • P₁ = 0.98 atm

Colocando los datos:

  • 294.16 K * P₂ = 310.16 K * 0.98 atm

Y <u>despejando P₂</u>:

  • P₂ = 1.03 atm
7 0
2 years ago
3 A roller coaster car travels up a hill until it reaches the top, slowly goes over, and speeds down the hill and through the nu
STALIN [3.7K]

Answer:

3rd law

Explanation:

8 0
3 years ago
Use the mass and volume data to calculate the density of mercury to the nearest tenth. Mass of mercury = 57 g Volume of mercury
Elena-2011 [213]

Density = mass/volume = 57g/4.2 mL ≈ 13.6 g/mL

7 0
3 years ago
Read 2 more answers
Consider the following Reaction.
Evgen [1.6K]

Answer: -

O 2 limiting reagent

53.83 g CO2 theoretical Yield

97.9% percentage yield

Explanation: -

Mas of CH4 = 23.2 g

Molar mass of CH4 = 12 x 1 + 1 x 4 = 16g

Mass of O2 = 78.3 g

Molar mass of O 2 – 16 x 2 = 32 g

The balanced chemical equation for the reaction is

CH4 + 2 O2 = CO2 + 2 H2O

From the balanced equation we see that

2 O 2 reacts with 1 CH4

2 x 32 g of O 2 react with 16 g of CH4

78.3 g of O 2 react with \frac{16 g CH4 x 78.3 g O2}{2 x32 g O2}

= 19.575 g pf CH4

Thus CH4 is in excess.

The limiting reagent is thus O 2.

Molar mass of CO2 = 12 x 1 + 16 x 2= 12 +32 = 44g

From the balanced equation we see

2O 2 gives 1 CO2

2 x 32 g of O 2 gives 44g of CO2

78.3 g of O 2 gives = \frac{44 gCO2 x 78.3 g O2}{2 x 32 g O2}

=53.83 g of CO2

Theoritical Yield = 53.83 g of CO2

Actual yield = 52.7 g

Percentage yield = \frac{52.7 g}{53.83 g} x 100

=97.9 %

5 0
3 years ago
The solubility of a gas in water is 0.16g/L at 104 kPa. What is the solubility when the pressure of the gas is increased to 288
stepladder [879]
Answer:
new solubility = 0.443 g/l

Explanation:
To solve this question, we will use Henry's law.
Henry's law states that, at constant temperature:
S1 / P1 = S2 / P2

We are given that:
S1 = 0.16 g/l
P1 = 104 kPa
S2 is the solubility we want to calculate
P2 = 288 kPa

Substitute with the givens in the above relation to get the new solubility (S2) as follows:
0.16 / 104 = S2 / 288
S2 = (0.16/104) * 288
S2 = 0.443 g/l

Hope this helps :)

7 0
2 years ago
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