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What does the kinetic theory state?

LUCKY_DIMON [66]

Answer:

Explanation:

Kinetic molecular theory of gasses stated that,

1) Gases consist of large number of smaller particles which are distance apart from each others.

2) The gas molecules collide with each other and also with wall of container and this collision is elastic.

3) Gas molecules are in continuous random motion and posses kinetic energy.

4) The forces of attraction between gas molecules are very small and considered negligible.

5) The temperature of gas is directly proportional to average kinetic energy of gas molecules.

8 0

3 years ago

Calculate the volume, in milliliters, of a 0.211 M solution of NaOH that will completely neutralize each of the following. 2.30

xenn [34]

Answer:

$V_{base}=17.9mL$

Explanation:

Hello,

In this case, as the reaction between sodium hydroxide and sulfuric is:

$2NaOH+H_2SO_4\rightarrow Na_2SO_4+2H_2O$

We can notice a 2:1 molar ratio between the base and the acid, for that reason for the titration at the equivalence point we find:

$n_{base}=2*n_{acid}$

Which in terms of concentrations and volumes is:

$M_{base}V_{base}=2*M_{acid}V_{acid}$

In such a way, solving for the required volume of base we find:

$V_{base}=\frac{2*M_{acid}V_{acid}}{M_{base}} \\\\V_{base}=\frac{2*0.820M*2.30mL}{0.211M}\\ \\V_{base}=17.9mL$

Best regards.

7 0

3 years ago

What mass of water is produced when 425 g of octane is burned?

Vitek1552 [10]

659. 48 g of water is produced

3 0

3 years ago

Glucose is soluble in water. Why is cellulose, which is made up of glucose, insoluble in water?

lapo4ka [179]

.....................

3 0

3 years ago

A student mixes a 10.0 mL sample of 1.0 M NaOH with a 10.0 mL sample of 1.0 M HCl in a polystyrene container. The temperature of

ElenaW [278]

Answer:

The experimental value of ΔH is -50 kJ/mol

Explanation:

Step 1: Data given

Volume of 1.0 M NaOH = 10.0 mL = 0.01 L

Volume of 1.0 M HCl = 10.0 mL = 0.01 L

Temperature before mixing = 20 °C

Final temperature = 26 °C

Specific heat of solution = 4.2 J/g°C

Density = 1g/mL

Step 2: Calculate q

q = m*c*ΔT

⇒ with m = the mass

⇒ 20.0 mL * 1g/mL = 20 grams

⇒ c = specific heat of solution = 4.2 J/g°C

⇒ ΔT = T2 -T1 = 26 -20 = 6 °C

q = 20g * 4.2 J/g°C * 6°C

q = 504 J

ΔHrxn = -q ( because it's an exothermic reaction)

ΔHrxn = -504 J

Step 3: Calculate number of moles

Moles = Molarity * volume

Moles = 1M *0.01 L = 0.01 moles

Step 4: Calculate the experimental value of ΔH

ΔHrxn = -504 / 0.01 mol = -50400 J/mol = -50.4 kJ/mol

The experimental value of ΔH is -50 kJ/mol

6 0

4 years ago