Which factors were affected by the breakup of the supercontinent Pangaea? Check all that apply.

How many moles are present in 16.9 g of Al2O3?

Dahasolnce [82]

The number of moles in Al2O3 is .16575 moles

4 0

3 years ago

Im doing a science project and need examples and non-examples of an Atom. some examples of an atom is neon, hydrogen, argon, etc

gogolik [260]

Answer:

Anything not on the periodic table is an element non example! ... So, for a substance to be an element, all of its atoms must have the same number of protons. Examples of elements include hydrogen, lithium, nickel, and radium.

Explanation:

6 0

3 years ago

g How many moles of NaOH are present in a sample if it is titrated to its equivalence point with 44.02 mL of 0.0885 M H2SO4? 2Na

Lisa [10]

Answer:

$n_{base}=3.90x10^{-3}molNaOH$

Explanation:

Hello!

In this case, since the sulfuric acid and sodium hydroxide react in a 1:2 mole ratio, given the reaction, we realize they have the following mole ratio at the equivalence point:

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

Which in terms of concentrations and volumes is:

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

Thus, we can plug in the volume and concentration of acid to find the moles of base:

$n_{base}=0.04402L*0.0885\frac{mol}{L} \\\\n_{base}=3.90x10^{-3}molNaOH$

Best regards!

8 0

3 years ago

How much of glucose (C6H1206) is needed to make 1 L of a 1-M solution? Use details to support your answer.

Yakvenalex [24]

Answer:

200 g C₆H₁₂O₆

General Formulas and Concepts:

Chemistry - Solutions

Reading a Periodic Table
Using Dimensional Analysis
Molarity = moles of solute / liters of solution

Explanation:

Step 1: Define

1 M C₆H₁₂O₆

1 L of solution

Step 2: Identify Conversions

Molar Mass of C - 12.01 g/mol

Molar Mass of H - 1.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar mass of C₆H₁₂O₆ - 6(12.01) + 12(1.01) + 6(16.00) = 180.18 g/mol

Step 3: Find moles of solute

1 M C₆H₁₂O₆ = x mol C₆H₁₂O₆ / 1 L

x = 1 mol C₆H₁₂O₆

Step 4: Convert

$1 \ mol \ C_6H_{12}O_6(\frac{180.18 \ g \ C_6H_{12}O_6}{1 \ mol \ C_6H_{12}O_6} )$ = 180.18 g C₆H₁₂O₆

Step 5: Check

We are given 1 sig figs. Follow sig fig rules and round.

180.18 g C₆H₁₂O₆ ≈ 200 g C₆H₁₂O₆

3 0

3 years ago

What is the quantity of heat (in kJ) associated with cooling 185.5 g of water from 25.60°C to ice at -10.70°C?Heat Capacity of S

Cerrena [4.2K]

Taking into account the definition of calorimetry, sensible heat and latent heat, the amount of heat required is 37.88 kJ.

<h3>Calorimetry</h3>

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

<h3>Sensible heat</h3>

Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

<h3>Latent heat</h3>

Latent heat is defined as the energy required by a quantity of substance to change state.

When this change consists of changing from a solid to a liquid phase, it is called heat of fusion and when the change occurs from a liquid to a gaseous state, it is called heat of vaporization.

25.60 °C to 0 °C

First of all, you should know that the freezing point of water is 0°C. That is, at 0°C, water freezes and turns into ice.

So, you must lower the temperature from 25.60°C (in liquid state) to 0°C, in order to supply heat without changing state (sensible heat).

The amount of heat a body receives or transmits is determined by:

Q = c× m× ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

In this case, you know:

c= Heat Capacity of Liquid= 4.184 $\frac{J}{gC}$
m= 185.5 g
ΔT= Tfinal - Tinitial= 0 °C - 25.60 °C= - 25.6 °C

Replacing:

Q1= 4.184 $\frac{J}{gC}$ × 185.5 g× (- 25.6 °C)

Solving:

Q1= -19,868.98 J

Change of state

The heat Q that is necessary to provide for a mass m of a certain substance to change phase is equal to

Q = m×L

where L is called the latent heat of the substance and depends on the type of phase change.

In this case, you know:

n= 185.5 grams× $\frac{1mol}{18 grams}$ = 10.30 moles, where 18 $\frac{g}{mol}$ is the molar mass of water, that is, the amount of mass that a substance contains in one mole.