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Lunna [17]
3 years ago
5

Given 40 grams of magnesium. How many mole is this

Chemistry
1 answer:
Dahasolnce [82]3 years ago
3 0

To determine the moles in 40 grams of magnesium, we need the atomic weight. This can easily be found on a periodic table. For this problem, let's use 24.305 grams/mole.

We are going to set up an equation to determine this problem. In this equation, we want all our units to cancel out except for 'moles.'

\frac{40 g Mg}{1} x\frac{1 mole Mg}{24.305 g Mg}

In this, we can see that the unit 'grams' will cancel out to leave us with moles.

In solving the equation, we determine that there are approximately 1.65 moles of Magnesium.

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horrorfan [7]

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<h3>what are the development and characterization of Carbon Nanofiber for Additively Manufactured Piezo resistive Sensors?</h3>

In accordance with the semiconductor material's piezo resistive effect, diffusion resistance is used to manufacture piezo resistive sensors on substrates of semiconductor materials. The diffusion resistor is connected in the substrate in the form of a bridge, allowing the substrate to be employed directly as a measuring sensor element.

  • Carbon nanofiber/polylactic acid filament for fused filament fabrication (FFF) and additive manufacturing (AM) strain sensors was studied for the effects of production factors.
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5 0
1 year ago
Calculate the solubility of ( = ) in moles per liter. Ignore any acid–base properties. s = mol/L Calculate the solubility of ( =
BaLLatris [955]

This is an incomplete question, here is a complete question.

Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid-base properties.

CaCO₃, Ksp = 8.7 × 10⁻⁹

Answer : The solubility of CaCO₃ is, 9.33\times 10^{-5}mol/L

Explanation :

As we know that CaCO₃ dissociates to give Ca^{2+} ion and CO_3^{2-} ion.

The solubility equilibrium reaction will be:

CaCO_3\rightleftharpoons Ca^{2+}+CO_3^{2-}

The expression for solubility constant for this reaction will be,

K_{sp}=[Ca^{2+}][CO_3^{2-}]

Let solubility of CaCO₃ be, 's'

K_{sp}=(s)\times (s)

K_{sp}=s^2

8.7\times 10^{-9}=s^2

s=9.33\times 10^{-5}mol/L

Therefore, the solubility of CaCO₃ is, 9.33\times 10^{-5}mol/L

4 0
3 years ago
Calculate the boiling temperature of a 0.50 M solution of sucrose. Assume that the concentration is 0.50 m.
Ronch [10]
There is one missing point in the question.

The formula to find an increase in boiling Temperature is :

ΔT = kb x M

ΔT = is the increase in boiling Temperature
Kb = Boiling point constant of the Solvent
M = Molarity

You did not provide the Kb. If you have it, you just have to insert it to the formula to find the ΔT.


And assuming that the other solution is water, you just have to add it up with 100 Celcius


5 0
3 years ago
HELP! ASAP! Iron (Fe) and copper (II) chloride (CuCl2) combine to form iron (III) chloride (FeCl3) and copper (Cu). If you start
Helga [31]

Answer: 30.978

Explanation:

From the equation 2 moles of Fe will result in 3 moles copper

so .325 moles Fe will result in .4875 moles Cu

Cu weights 63.546 gm per mole

.4875 moles * 63.546 gm / mole = 30.978 gm of Cu

7 0
2 years ago
If 0.500 mol neon at 1.00 atm and 273 K expands against a constant external pressure of 0.100 atm until the gas pressure reaches
trapecia [35]

Answer:

The work done on neon = -323 J

The internal energy change= -392.84 J

The heat absorbed by neon = -69.84 J

Explanation:

Step 1: Data given

Number of moles  = 0.500 moles

Pressure  = 1 atm

Temperature  = 273 Kelvin

The pressure will change from 1.00 atm to 0.200 atm. The temperature changes from 273 to 210 Kelvin.

a) calculate the work done on neon

W = -P(V2-V1)    

⇒ with P = the pressure = 0.1 atm

⇒ with V1 = the initial volume = nRTi /Pi

⇒ with V2 = the final volume = nRTf /Pf

W = -PnR((T2/P2) -(T1/P1))

⇒ with T2 = the final temperature = 210 K

 ⇒ with T1 = the initial temperature = 273 K

 ⇒ with P2 = the final pressure = 0.200 atm

 ⇒ with P1 = the initial pressure = 1.00 atm

W = -nR (210*(0.1/0.2) - 273*(0.1/1.00))

W = -nR*(105 - 27.3)

W= -(0.500)*(8.314)*(77.7)

W = -323 J

b) calculate the internal energy change

E = (3/2)*nRT

ΔE = Ef - Ei

ΔE =(3/2)*nR(T2-T1)

⇒ with n= number of moles = 0.500 moles

⇒ with T2 =the final temperature = 210 K

⇒ with T1 = the initial temperature = 273 K

ΔE = (3/2)*(0.5)*(8.314)(210-273)

ΔE = -392.84 J

c) Calculate the heat absorbed by neon

ΔE = q + W

q = ΔE -W

⇒ with ΔE = -392.84 J

⇒ with W = -323 J

q = -392.84 J -( -323 J)

q =-392.84 J + 323 J

q = -69.84 J

4 0
3 years ago
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