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Lapatulllka [165]
3 years ago
8

Which unit is used for measuring atomic mass?

Chemistry
1 answer:
katrin2010 [14]3 years ago
5 0
The answer is Atomic Mass unit (Amu)
One unified atomic mass is numerically equivalent to 1 g/mol and  is equal to  the mass of one nucleon.
To describe atomic mass, it is also common to use Dalton as similar unit measurement as a form of respect to his works in Atom.
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Antarctica, almost completely covered in ice, has an area
Marysya12 [62]

<u>Answer:</u> The mass of ice is 2.39\times 10^{22}g

<u>Explanation:</u>

We are given:

Area of Antarctica = 5,500,000mi^2=5,500,000\times 2.59\times 10^{10}=142.45\times 10^{15}cm^2      (Conversion factor:  1mi^2=2.59\times 10^{10}cm^2  )

Height of Antarctica with ice = 7500 ft.

Height of Antarctica without ice = 1500 ft.

Height of ice = 7500 - 1500 = 6000 ft = 182.88\times 10^3cm     (Conversion factor:  1 ft = 30.48 cm)

To calculate mass of ice, we use the equation:

\text{Density of a substance}=\frac{\text{Mass of a substance}}{\text{Volume of a substance}}

We are given:

Density of ice = 0.917g/cm^3

Volume of ice = Area × Height of ice = 142.45\times 10^{15}cm^2\times 182.88\times 10^3cm=26051.26\times 10^{18}cm^3

Putting values in above equation, we get:

0.917g/cm^3=\frac{\text{Mass of ice}}{26051.26\times 10^{18}cm^3}\\\\\text{Mass of ice}=(0.917g/cm^3\times 26051.26\times 10^{18}cm^3=2.39\times 10^{22}g

Hence, the mass of ice is 2.39\times 10^{22}g

5 0
3 years ago
If you have 60 grams of MgCl2 in 5 liters of solution, what is the molarity of this solution?
AnnyKZ [126]

Answer:

molarity =gram/litre

=60/5

12

6 0
3 years ago
15 points will mark brainliest
AfilCa [17]
Part B question 1 Answer: C
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6 0
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Liquidtight flexible nonmetallic conduit marked as ____ has a smooth seamless inner core and cover bonded together and one or mo
DanielleElmas [232]

Answer:

LFNC-A

Explanation:

Liquidtight Flexible Non-Metallic Conduit Type LFNC-A is a layered raceway of circular cross section with a smooth flexibly polyvinyl chloride (PVC) inner layer with a reinforcing layer covered with a flexible polyvinyl chloride (PVC) jacket.

5 0
3 years ago
You want to determine ΔH o for the reaction Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) To do so, you first determine the heat capacity
Assoli18 [71]

Answer:

(A) The heat capacity of the calorimeter is therefore = −2.1428KJ÷13.5°C

= −0.1587KJ/°C

 

(B) ΔHo for the reaction Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) = –15.42KJ

Explanation:

Solution

 

Calculate the heat actually evolved.

                 q = mcΔt

 

Finding the mass of the reactants in grams we have.

 

Use density. (50 mL + 50 mL ) = 100 mL of solution.

 

100 mL X 1.04g/mL     = 104 grams of solution. (mass = Volume X Density)

                       

 

Find the temperature change.

 

       Δt =tfinal - tinitial = 30.4°C – 16.9°C = 13.5°C

 

    q = mcΔt

       = 104grams × 3.93J/g°C  × 13.5°C = 5.51772×103J

                                         

 

       = 5.51772 × 103 J

 

This is the heat lost in the reaction between HCl and NaOH, therefore q = -5.52 × 103 J.

 

this is an exothermic heat producing reaction.

 To calculate the total heat of the reaction or heat per mole we have

  

50.0 mL of HCl X 2.00 mol HCl /(1000 mL HCl ) = 0.100 mol HCl

                            

 

The same quantity of base, 0.100 mole NaOH, was used.

The energy per unit mole is given by

  

i.e. molar enthalpy = J/mol = -5.52 × 103J / 0.100 mol

            = -5.52 × 104 J/mol

            = -55177.2 J/mol

            = -55.177 kJ/mol

 

Therefore, the enthalpy change for the neutralization of HCl and NaOH, that is the enthalpy, heat, of reaction is ΔH = -55.177 kJ/mol

Heat absorbed by the calorimeter = −57.32kJ − 55.177 kJ = −2.1428KJ

The heat capacity of the calorimeter is therefore = −2.1428KJ÷13.5°C

= −0.1587KJ/°C

 

(B) For the ZnCl we have

 

Calculate the heat actually evolved.

                            q = mcΔt

 

Finding the mass of the reactants in grams we have.

 

Use density.  100 mL of solution of HCl

 

100 mL X 1.015g/mL        = 101.5 grams of solution. (mass = Volume X Density)

                       

 

Find the temperature change.

 

       Δt =tfinal - tinitial = 20.5°C – 16.8°C = 3.7 °C

 

    q = mcΔt

       = 101.5grams × 3.95J/g°C  × 3.7°C = 1483.422×103J

                                         

 

       = -1483.422×103J

 

This is the heat lost in the reaction between HCl and NaOH, therefore q = -1.483 × 103 J.

 

this is an exothermic heat producing reaction.

 To calculate the total heat of the reaction or heat per mole we have

  

100.0 mL of HCl X 1.00 mol HCl /(1000 mL HCl ) = 0.100 mol HCl

                            

 

 

The energy per unit mole is given by

  

i.e. molar enthalpy = J/mol = -1.483 × 103J / 0.100 mol

                                         = -1.483 × 104 J/mol

                                         = -14834.22 J/mol

                                         = -14.834 kJ/mol

 

Therefore, the enthalpy change for the neutralization of HCl and NaOH, that is the enthalpy, heat, of reaction is ΔH = -14.834 kJ/mol

ΔHo for the reaction Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)

= -14.834 kJ –(0.1587KJ/°C×3.7°C) = -15.42KJ

ΔHo for the reaction Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) = –15.42KJ

5 0
3 years ago
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