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3 years ago

14 Which property is a measure of the average kinetic energy of the particles in a sample or matter?

1 answer:

3 0

(4) temperature is the correct answer.

Average kinetic energy is calculated by 3/2*R*T, in which R is a constant and is equal to 8.3145 J/ mol*K, and T is temperature measured in Kelvins.

Hope this helps~

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Four people weigh a standard mass of 10.00g on the same balance. Which of the following sets of readings suggests measurements t

Svetach [21]

An example of accurate but not precise would be 3 people weigh a 10g sample. the weights are 0g, 10g, & 20 grams. the scale is way off but the weights average to the right thing.
precise but not accurate would weighing a 10g sample 3 times and getting 5.5, 5.4, & 5.5. they'e all incredibly similar therefore precise but its nowhere near 10, so not accurate.
neither precise nor accurate would be 3 weights being 10, 20, &30. It averages wrong and is imprecise.

5 0

3 years ago

Write the correct name of the Fe(CIO3)3

pychu [463]

Answer:

Iron(III) Chlorate Fe(ClO3)3 Molecular Weight

Explanation:

3 0

1 year ago

Read 2 more answers

What is chemical formula and equation ?

Daniel [21]

The answer to your question is,

Chemical formula is "a mathematical relationship or rule expressed in symbols". For example, H2 + O = H2O. < Water.

The equation H2 + O = H2O is two elements combining together. H, hydrogen. O, Oxygen. They form together to make a new compound of elements. Water. :))

-Mabel <3

8 0

3 years ago

If 18.1 g of ammonia is added to 27.2 g of oxygen gas, how many grams of excess reactant is remaining once the reaction has gone

GREYUIT [131]

Answer:

m of NH3 = 6.46 g

Explanation:

First, in order to know the limiting and excess reactant, we need to write and balance the equation that is taking place:

NH₃ + O₂ ---------> NO + H₂O

Now, let's balance the equation:

4NH₃ + 5O₂ ---------> 4NO + 6H₂O

Now that we have the balanced equation, let's see which reactant is in excess. To know that, let's calculate the moles of each reactant using the molar mass:

MM NH3 = 17 g/mol

MM O2 = 32 g/mol

moles NH3 = 18.1 / 17 = 1.06 moles

moles O2 = 27.2 / 32 = 0.85 moles

Now, let's compare these moles with the theorical moles that the balanced equation gave:

4 moles NH3 --------> 5 moles O2

1.06 moles ----------> X

X = 1.06 * 5 / 4 = 1.325 moles of O2

These means in order to NH3 completely reacts with O2, it needs 1.325 moles of O2, which we don't have it. We only have 0.85 moles of O2, therefore, the limiting reactant is the O2 and the excess is NH3.

Now, let's see how many grams in excess we have left after the reaction is complete.

4 moles NH3 --------> 5 moles O2

X moles NH3 ----------> 0.85 moles

X = 0.85 * 4 / 5 = 0.68 moles of NH3

This means that 0.85 moles of O2 will react with only 0.68 moles of NH3, and we have 1.06 so, the remaining moles are:

moles remaining of NH3 = 1.06 - 0.68 = 0.38 moles

Finally the mass:

m = 0.38 * 17

8 0

2 years ago

The elementary reaction 2 H 2 O ( g ) − ⇀ ↽ − 2 H 2 ( g ) + O 2 ( g ) proceeds at a certain temperature until the partial pressu

Andru [333]

Answer:

6.72 × 10⁻⁴

Explanation:

Let's consider the following elementary reaction.

2 H₂O(g) ⇄ 2 H₂(g) + O₂(g)

The equilibrium constant (Kp) is the product of the partial pressures of the products raised to their stoichiometric coefficients divided by the product of the partial pressures of the reactants raised to their stoichiometric coefficients.

$Kp=\frac{pH_{2}^{2}.pO_{2} }{pH_{2}O^{2} } =\frac{(0.00550)^{2}.(0.00500)}{(0.0150)^{2} } =6.72 \times 10^{-4}$

4 0

3 years ago