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4 years ago

A gas has pressure of 50.0 mmHG at a temperature of 540K. What will be the temperature if the pressure goes down to 3 mmHG

Chemistry

1 answer:

Sonja [21]4 years ago

5 0

Answer:

32.4 K

Explanation:

From the given parameters;

Initial pressure P1= 50.0 mmHg

Initial temperature T1= 540K

Final Temperature T2 = ?????

Final pressure P2=3 mmHg

Now using this relationship;

P1/T1 = P2/T2

We have; P1T2= P2T1

Hence;

T2= P2T1/P1

T2= 3 ×540/50.0

T2= 32.4 K

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kompoz [17]

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7 0

3 years ago

I need help what is s-1/3=7/9???? please help guys and thank you

nalin [4]

Answer:

10/9

Explanation:

First, let's convert 1/3 and 7/9 so that the have the same denominator. To do this let's find the least common multiple of 3 and 9.

List the multiples of 3 and 9:

3: 3, 9

9: 9

They have a least common multiple of 9

We need to convert 1/3 so it has a denominator of 9:

1/3*3/3 (we can multiply it by 3/3 because any number over itself is 1) = 3/9

s-3/9=7/9

Add 3/9 to both sides to isolate s

s=10/9

6 0

3 years ago

Nitrogen gas makes up more of the atmosphere than any other type of molecule.

Ad libitum [116K]

Nitrogen gas makes up more of the atmosphere than any other type of molecule.

N2

5 0

4 years ago

If 1.240 g of carbon dioxide dissolves in 1.01 l of water at 755 mm hg, what quantity of carbon dioxide (in grams) will dissolve

Lelu [443]

Answer : 1.297 g carbon dioxide will dissolve at 790 mm Hg

Explanation :

According to Henry's law, the amount of gas dissolved in water at a given temperature is directly proportional to its vapor pressure .

In equation format the law can be written as

$C_{gas}= K\times P_{gas}$

Here C is the concentration of the gas

P is the partial pressure of the gas

K is known as Henry's constant which is temperature dependent.

At 2 different partial pressure values, the equation can be modified as follows

$\frac{C_{1}}{C_{2}}= \frac{P_{1}}{P_{2}}$

Let us calculate C₁

C₁ = amount of gas in grams / L

C₁ = 1.240 g / 1.01 L

C₁ = 1.228 g/L

P₁ = 755 mm Hg

P₂ = 790 mm Hg

C₂ = ?

Let us plug in the values in Henry's equation

1.228 g L⁻¹ / C₂ = 755 mm Hg / 790 mm Hg

1.228 g L⁻¹ / C₂ = 0.956

C₂ = 1.228 g L⁻¹ / 0.956

C₂ = 1.285 g L⁻¹

The concentration of carbon dioxide at 790 mm Hg is 1.285 g/L

We have 1.01 L water.

Therefore the amount of gas dissolved = 1.01 L x 1.285 g/L = 1.297 g

1.297 g carbon dioxide will dissolve at 790 mm Hg in 1.01 L water

7 0

3 years ago

Read 2 more answers

Calculate the concentration of acetate ion in a buffer solution made from 2.00 mL of 0.50 M acetic acid and 8.00 mL of 0.50 sodi

Lelu [443]

Answer:

1 M

Explanation:

Equation of reaction is;

CH3COOH + CH3COONa -------------------> 2CH3COO^- + NaH

1 moles of each of the reactants react to give 2 moles of the acetate ion.

From the question, we have that 2.00 mL that is (2÷1000)L of 0.50 M acetic acid reacted with 8.00 mL that is (8/1000)L of 0.50 sodium acetate.

Then from equation, n = CV -------------------------------------------(1).

Where n= number of moles, V= volume, C= concentration.

Number of moles,n of acetic acid = 0.50M× 2/1000L.

n(acetic acid)= 0.001 moles.

Number of moles,n of sodium acetate= 0.50M ×(8/1000)L.

n(sodium acetate)= 0.004 moles.

0.001 moles of acetic acid react with 0.004 moles of Sodium acetate

Therefore, acetic acid is the limiting reagent.

One mole of acetic acid produces 2 moles of acetate ion.

0.001 mole of acetic acid produces= 0.002 moles of acetate ion.

Using the equation (1) that is, n= CV.

0.002= C× 2/1000

C= 0.002/0.002

C= 1 M

8 0

4 years ago