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8_murik_8 [283]
3 years ago
10

What is the molar mass of H2(SO4)3?​

Chemistry
1 answer:
nalin [4]3 years ago
7 0

Answer:

Explanation:

The molecular mass of C2H6 is approximately 30 or [(2 x 12) + (6 x 1)]. Therefore the molecule is about 2.5 times as heavy as the 12C atom or about the same mass as the NO atom with a molecular mass of 30 or (14+16).

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777 Joules of energy are applied to 25.0 grams of each of the following materials, which
4vir4ik [10]

Answer:

I think copper

Explanation:

Material IACS % Conductivity

Silver                105

Copper            100

Gold               70

Aluminum         61

Nickel              22

Zinc                          27

Brass                  28

Iron                        17

Tin                      15

Phosphor Bronze  15

Lead                      7

Nickel Aluminum Bronze 7

Steel                   3 to 15

the table might help- your indian brother

3 0
2 years ago
How many electrons does H have with a -1 charge
pentagon [3]

Answer:The electron has a negative charge and the proton has a positive charge, and these charges work against each other to make the electromagnetic force that holds the entire atom together.

Explanation:

This is the answer

5 0
3 years ago
An aqueous solution of sodium
DochEvi [55]

Answer:

2.5×10^-7mol/dm^3

Explanation:

Firstly convert the cm^3 to dm^3

200×1000=200000dm^3

Calculate the g/dm^3

2/200000=0.00001g/dm^3

To calculate mol/dm^3

Mol/dm^3=mass given\molar mass

=0.00001/40

=2.5×10^-7mol/dm^3

8 0
3 years ago
Read 2 more answers
Could the structures below undergo a Fischer esterification reaction? Reaction scheme of benzoic acid and thionyl chloride to fo
Romashka-Z-Leto [24]

Answer:

The correct answer is the first option. No, the structures above cannot undergo a Fischer esterification reaction to form an ester.

Explanation:

The reaction that will take place can be found in the attached file. The reaction does not require any catalyst and it cannot undergo a Fischer esterification reaction to form an ester.

4 0
3 years ago
15.0 moles of gas are in a 8.00 L tank at 22.3 ∘C∘C . Calculate the difference in pressure between methane and an ideal gas unde
leva [86]

Answer:

\Delta P=4.10atm

Explanation:

Hello!

In this case, since the ideal gas equation is used under the assumption of no interaction between molecules and perfectly sphere-shaped molecules but the van der Waals equation actually includes those effects, we can compute each pressure as shown below, considering the temperature in kelvins (22.3+273.15=295.45K):

P^{ideal}=\frac{nRT}{V}=\frac{15.0mol*0.08206\frac{atm*L}{mol*K}*295.45K}{8.00L}=45.5atm

Next, since the VdW equation requires the molar volume, we proceed as shown below:

v=\frac{8.00L}{15.0mol}=0.533\frac{L}{mol}

Now, we use its definition:

P^{VdW}=\frac{RT}{v-b} -\frac{a}{v^2}

Thus, by plugging in we obtain:

P^{VdW}=\frac{0.08206\frac{atm*L}{mol*K}*295.45K}{0.533mol/L-0.0430L/mol} -\frac{2.300L^2*atm/mol^2}{(0.533L/mol)^2}\\\\P^{VdW}=49.44atm-8.09atm\\\\P^{VdW}=41.4atm

Thus, the pressure difference is:

\Delta P=45.5atm-41.4atm\\\\\Delta P=4.10atm

Best regards!

6 0
3 years ago
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