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3 years ago

Help me pls its chemistry

Chemistry

1 answer:

saul85 [17]3 years ago

8 0

B to C:-

The temperature remains constant from B to C in any time interval .
Looking at the graph there is BC || x axis.
Hence temperature remains unchanged.

E to D:-

Here also the temperature remains constant.
As we can see ED|| x axis

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The table below gives the equilibrium concentrations for this reaction at a certain temperature : N2(g) + O2(g) 2NO(g) what is t

makkiz [27]

D. 100 I hope this help :)

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3 years ago

What is the concentration of the barium hydroxide solution if 50.0 mL of a 0.425 M HNO3 solution is required to neutralize a 36.

fomenos

The molarity of Barium Hydroxide is 0.289 M.

Explanation:

We have to write the balanced equation as,

Ba(OH)₂ + 2 HNO₃ → Ba(NO₃)₂ + 2 H₂O

We need 2 moles of nitric acid to react with a mole of Barium hydroxide, so we can write the law of volumetric analysis as,

V1M1 = 2 V2M2

Here V1 and M1 are the volume and molarity of nitric acid

V2 and M2 are the volume and molarity of Barium hydroxide.

So the molarity of Ba(OH)₂, can be found as,

$$ M2 = \frac{V1 \times M1}{2 \times V2}$

$$M2 = \frac{50 \times 0.425 }{2 \times 36.8}$

= 0.289 M

5 0

3 years ago

240 g of water (specific heat = 4.186 J/g°C, initial temperature = 20°C) is mixed with an

ivolga24 [154]

The answer for this would be 69.6

3 0

3 years ago

Hydrogen produced from a hydrolysis reaction was collected over water and the following data was compiled.

Shkiper50 [21]

Answer:

0.00358 mol

Explanation:

1) Data:

a) V = 93.90 ml

b) T = 28°C

c) P₁ = 744 mmHg

d) P₂ = 28.25 mmHg

d) n = ?

2) Conversion of units

a) V = 93.90 ml × 1.000 liter / 1,000 ml = 0.09390 liter

b) T = 28°C = 28 + 273.15 K = 301.15 K

c) P₁ = 744 mmHg × 1 atm / 760 mmHg = 0.9789 atm

d) P₂ = 28.5 mmHg × 1 atm / 760 mmHg = 0.0375 atm

3) Chemical principles and formulae

a) The total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas. Hence, the partical pressure of the hydrogen gas collected is equal to the total pressure less the vapor pressure of water.

b) Ideal gas equation: pV = nRT

4) Solution:

a) Partial pressure of hydrogen gas: 0.9789 atm - 0.0375 atm = 0.9414 atm

b) Moles of hygrogen gas:

pV = nRT ⇒ n = pV / (RT) =

n = (0.9414 atm × 0.09390 liter) / (0.0821 atm-liter /K-mol × 301.15K) =

n = 0.00358 mol (which is rounded to 3 significant figures) ← answer

7 0

3 years ago

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Amiraneli [1.4K]

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3 years ago