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3 years ago

Which of the following best defines the internal energy of a system?

1 answer:

7 0

In thermodynamics, the internal energy of a thermodynamic system, or a body with well-defined boundaries, denoted by U, or sometimes E, is the total of the kinetic energy due to the motion of molecules (translational, rotational, vibrational) and the potential energy associated with the vibrational and electric energy of atoms within molecules or crystals. It includes the energy in all the chemical bonds, and the energy of the free, conduction electrons in metals.

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What is the voltage for the following cell: Cu(s)| Cu+(aq) || Mg2+(aq) |Mg(s)?

Julli [10]

Answer:

I think it is number 4 which is 3.87 v

6 0

3 years ago

Select the correct answer. if two half-lives have passed since a scientist collected a 1.00-gram sample of u-235, how much u-235

Ugo [173]

Answer:

0.25 g of U-235 isotope will left .

Formula used :

where,

N = amount of U-235 left after n-half lives = ?

= Initial amount of the U-235 = 1.00 g

n = number of half lives passed = 2

0.25 g of U-235 isotope will left .

3 0

2 years ago

Consider the generic reaction: 2 A(g) + B(g) → 2 C(g). If a flask initially contains 1.0 atm of A and 1.0 atm of B, what is the

irina1246 [14]

Answer:

b. 1.5 atm.

Explanation:

Hello!

In this case, since the undergoing chemical reaction suggests that two moles of A react with one moles of B to produce two moles of C, for the final pressure we can write:

$P=P_A+P_B+P_C$

Now, if we introduce the stoichiometry, and the change in the pressure $x$ we can write:

$P=1.0-2x+1.0-x+2x$

Nevertheless, since the reaction goes to completion, all A is consumed and there is a leftover of B, and that consumed A is:

$x=\frac{1.0atm}{2}=0.5atm$

Thus, the final pressure is:

$P=1.0-2(0.5)+1.0-(0.5)+2(0.5)\\\\P=1.5atm$

Therefore the answer is b. 1.5 atm.

Best regards!

3 0

3 years ago

Convert 9.32x 10 23ª atoms of au to moles of au

7nadin3 [17]

Answer:

$\huge\boxed{\sf no.\ of\ moles = 1.55\ moles }$

Explanation:

Given:

Number of atoms = $9.32 \times 10^{23}$ atoms

Avogadro's Number = $6.023 \times 10^{23}$ atom / mol

Required:

Moles = ?

Formula:

$\displaystyle No.\ of\ moles = \frac{no. \ of \ atoms }{avogadro's \ no.}$

Solution:

$\displaystyle no. \ of \ moles = \frac{9.32\times 10^{23}}{6.023 \times 10^{23}}$

no. of moles = 1.55 moles

$\rule[225]{225}{2}$

Hope this helped!

5 0

3 years ago

What is the weight in grams of 3.36 x 10^23 molecules of copper sulfate

Llana [10]

Answer:

$m=89.0g$

Explanation:

Hello!

In this case, since we are given the formula units (molecules) of copper sulfate, it is possible to compute the moles of this compound via the Avogadro's number:

$n=3.36x10^{23}molecules*\frac{1mol}{6.022x10^{23}molecules}\\\\n=0.558mol$

Now, given the molar mass of copper sulfate which is 159.60 g/mol, the required mass in grams turns out:

$m=0.558mol*\frac{159.60g}{1mol}\\\\m=89.0g$

Best regards!

5 0

3 years ago