How many molecules are in 3.50 moles of NO2

Air masses carry their own weather.<br> True<br> False<br> The question is number 8

frozen [14]

True because I had the test

8 0

2 years ago

Vapor pressure can be described as: A) the temperature at which bubbles of vapor appear in a liquid. B) the pressure exerted on

Vanyuwa [196]

Answer: Option (D) is the correct answer.

Explanation:

Vapor pressure is defined as the pressure exerted by the vapors which are present on the surface of a liquid.

For example, vapor pressure of water at room temperature is 0.0313 atm.

On the other hand, the temperature at which the vapor pressure of a liquid equals atmospheric pressure is known as boiling point.

For example, boiling point of water at room temperature is $100^{o}C$ .

Thus, we can conclude that vapor pressure can be described as the pressure exerted by a gas above the surface of its liquid.

4 0

3 years ago

Classify each of the following properties as physical or chemical: A. Ice melts in the sun. B. Copper is a shiny metal. C. Paper

vampirchik [111]

Answer:

The answer to your question is below

Explanation:

Physical properties are the properties in which there is no change in the nature of the substance but there is a change in the physical state.

Chemical properties are the properties in which the substance changes its nature. A new substance is formed.

A. Ice melts in the sun. Physical p.

B. Copper is a shiny metal. Physical p.

C. Paper can burn. Chemical p.

D. A silver knife can tarnish. Physical p.

E. A magnet removes iron particles from a mixture. Physical p.

8 0

3 years ago

The teal line of the hydrogen emission spectrum has a wavelength of 486.0 nm. A hydrogen emission spectrum has a violet, a blue,

Sloan [31]

Answer:

The correct answer to the following question will be "4.08 × 10⁻¹⁹ Joule".

Explanation:

Given:

Wavelength, λ = 486.0 nm

As we know,

$E=h\upsilon =\frac{hc}{\lambda}$

On putting the estimated values, we get

⇒ $=\frac{1241.5 \ ev\ nm}{486 \ nm}$

⇒ $=2.554 \ ev$

∴ 1 ev = 1.6 × 10⁻¹⁹ J

Now,

Energy, $E=2.554\times 1.6\times 10^{-19}$

⇒ $=4.08\times 10^{-19} Joule$

7 0

2 years ago

A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup calorimeter fitted with a

worty [1.4K]

Answer:

THE ENTHALPY CHANGE IN KJ/MOLE IS +114 KJ/MOLE.

Explanation:

Heat = mass * specific heat capacity * temperature rise

Total volume = 100 + 50 = 150 mL

Total mass = density * volume

Total mass = 1 * 150 mL = 150 g

So therefore, the heat evolved during the reaction is:

Heat = 150 * 4.18 * ( 31.4 - 22.3)

Heat = 150 * 4.18 * 9.1

Heat = 5705.7 J

Equation for the reaction:

2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l)

From the equation, 2 moles of NaOH reacts with 1 mole of H2SO4 to produce 1 mole of Na2SO4 and 2 moles of water

50 mL of 1 M of H2SO4 contains

50 * 1 / 1000 mole of acid

= 0.05 mole of acid

The production of 1 mole of water evolved 5705.7 J of heat and hence the enthalpy changein kJ per mole will be:

0.05 mole of H2SO4 produces 5705.7 J of heat

1 mole of H2SO4 will produce 5705.7 / 0.05 J

= 114,114 J / mole

In kj/mole = 114 kJ/mole.

Hence, the enthalpy change of the reaction in kJ /mole is +114 kJ/mole.

5 0

3 years ago