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nata0808 [166]
3 years ago
12

11th grade chemistry question will mark brainliest

Chemistry
1 answer:
GaryK [48]3 years ago
5 0

Answer:

3.88 atm

Explanation:

We'll begin by calculating the number of mole of CO₂ in each case. This can be obtained as follow:

For 2.50 g of CO₂:

Mass of CO₂ = 2.5 g

Molar mass of CO₂ = 12 + (2×16) = 44 g/mol

Mole of CO₂ =?

Mole = mass / molar mass

Mole of CO₂ = 2.5 / 44

Mole of CO₂ = 0.06 mole

For 0.42 g of CO₂:

Mass of CO₂ = 2.5 g

Molar mass of CO₂ = 44 g/mol

Mole of CO₂ =?

Mole = mass / molar mass

Mole of CO₂ = 0.42 / 44

Mole of CO₂ = 0.010 mole

Finally, we shall determine the new pressure. This can be obtained as follow:

Initial mole (n₁) = 0.06 mole

Initial pressure (P₁) = 4.65 atm

Final mole (n₂) = 0.06 – 0.010 = 0.05 mole

Final pressure (P₂) =?

NOTE: Temperature and volume is constant.

P₁ / n₁ = P₂ / n₂

4.65 / 0.06 = P₂ / 0.05

Cross multiply

0.06 × P₂ = 4.65 × 0.05

0.06 × P₂ = 0.2325

Divide both side by 0.06

P₂ = 0.2325 / 0.06

P₂ = 3.88 atm

Thus, the new pressure is 3.88 atm.

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The pressure of a sample of argon gas was increased from 3.14 atm to 7.98 at a constant temperature. If the final volume of argo
noname [10]

Answer:

<h2>36.09 L</h2>

Explanation:

The initial volume can be found by using the formula for Boyle's law which is

P_1V_1 = P_2V_2

where

P1 is the initial pressure

P2 is the final pressure

V1 is the initial volume

V2 is the final volume.

Since we're finding the initial volume

V_1 =  \frac{P_2V_2}{P_1}  \\

We have

V_1 =  \frac{7.98 \times 14.2}{3.14} =   \frac{113.316}{3.14}  \\  = 36.0878...

We have the final answer as

<h3>36.09 L</h3>

Hope this helps you

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