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2 years ago

WILL MARK BRAINLIEST

Chemistry

1 answer:

Marysya12 [62]2 years ago

8 0

Answer:

8.28 × 10⁶ N

Explanation:

Step 1: Given data

Interior surface area of the habitat (S): 110 m²

Pressure in the habitat (P): 75.3 kPa

Step 2: Convert "P" to Pascal

We will use the conversion factor 1 kPa = 10³ Pa.

75.3 kPa × (10³ Pa/1 kPa) = 75.3 × 10³ Pa

Step 3: Calculate the total force exerted (F)

We will use the following expression.

P = F/S

F = P × S

F = 75.3 × 10³ Pa × 110 m²

F = 8.28 × 10⁶ N

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10 electrons

Explanation:

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3 years ago

How many milliliters of a 0.285 M HCl solution are needed to neutralize 249 mL of a 0.0443 M Ba(OH)2 solution?

meriva

Answer:

$\large \boxed{\text{77.4 mL}}$

Explanation:

Ba(OH)₂ + 2HCl ⟶ BaCl₂ + H₂O

V/mL: 249

c/mol·L⁻¹: 0.0443 0.285

1. Calculate the moles of Ba(OH)₂

$\text{Moles of Ba(OH)$_{2}$} = \text{0.249 L Ba(OH)}_{2} \times \dfrac{\text{0.0443 mol Ba(OH)}_{2}}{\text{1 L Ba(OH)$_{2}$}} = \text{0.011 03 mol Ba(OH)}_{2}$

2. Calculate the moles of HCl

The molar ratio is 2 mol HCl:1 mol Ba(OH)₂

$\text{Moles of HCl} = \text{0.011 03 mol Ba(OH)}_{2} \times \dfrac{\text{2 mol HCl}}{\text{1 mol Ba(OH)}_{2}} = \text{0.022 06 mol HCl}$

3. Calculate the volume of HCl

$V_{\text{HCl}} = \text{0.022 06 mol HCl} \times \dfrac{\text{1 L HCl}}{\text{0.285 mol HCl}} = \text{0.0774 L HCl} = \textbf{77.4 mL HCl}\\\\\text{You must add $\large \boxed{\textbf{77.4 mL}}$ of HCl.}$

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3 years ago

A first-order reaction has a half-life of 16.7 s . How long does it take for the concentration of the reactant in the reaction t

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It takes 33.4 s for the concentration of A to fall to one-fourth of its original value.

A <em>half-life</em> is the time it takes for the concentration to fall to half its original value.

Assume the initial concentration is 1.00 mol/L. Then,

$\text{1.00 mol/L }\stackrel{\text{1st half-life }}{\longrightarrow}\text{ 0.50 mol/L } \stackrel{\text{ 2nd half-life }}{\longrightarrow}\text{0.25 mol/L}\\$

The concentration drops to one-fourth of its initial value in two half-lives.

∴ Time = 2 × 16.7 s = 33.4 s

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3 years ago

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A sample of gas originally at 25 C and 1.00 atm pressure in a 2.5 L container is allowed to expand until the pressure is 0.85 at

aivan3 [116]

Answer:

Final volumeof the gas = 2.84 L

Explanation:

The formular to be used here is the general gas equation. the formular is being used because it gives the relationship between the three gas parameters (volume, temperature and pressure) mentioned.

The general gas equation is given as;

$\frac{P1V1}{T1} = \frac{P2V2}{T2}$

where;

P1 = initial pressure

V1 = initial volume

T1 = initial temperature

P2 = Final pressure

V2 = Final volume

T2 = Final temperature

From the question,

P1 = 1.00 atm

P2 = 0.85atm

T1 = 25C + 273 = 298K (Converting to kelvin)

T2 = 15C + 273 = 288K (Converting to kelvin)

V1 = 2.5L

V2 = ?

from the equation, making V2 subject of formula we have;

$V2 = \frac{T2P1V1}{T1P2}$

V2 = (1*2.5*288)/(298*0.85) = 2.84 L.

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3 years ago