Answer:
The correct option is: a. The internal energy depends upon its temperature.
Explanation:
Ideal gas is a hypothetical gas that obeys the ideal gas law. The equation for the ideal gas law:
P·V=n·R·T
Here, V- volume of gas, P - total pressure of gas, n- total mass or number of moles of gas, T - absolute temperature of gas and R- the gas constant
Also, according to the Joule's second law, the <em><u>internal energy (U) of the given amount of ideal gas depends on the absolute temperature (T) of the gas only,</u></em> by the equation:
Here, 
<em>is the specific heat capacity at constant volume</em>
There is no image , so you cannot answer , sorry
Answer is: d) Hg.
Mercury is a chemical element with the symbol Hg and atomic number 80. <span> Mercury is the only metallic element that is liquid at standard conditions for temperature and pressure.
</span>Absolute viscosity of mercury is 0,0015 Pa·s.
The viscosity<span> of a </span>fluid<span> is a measure of its </span>resistance<span> to gradual deformation by </span>shear stress<span> or </span><span>tensile stress</span>
Answer:
The radius of tantalum (Ta) atom is 
Explanation:
From the Body-centered cubic (BBC) crystal structure we know that a unit cell length <em>a </em>and atomic radius <em>R </em>are related through
So the volume of the unit cell 
is
We can compute the theoretical density ρ through the following relationship
where
n = number of atoms associated with each unit cell
A = atomic weight
= volume of the unit cell
= Avogadro’s number (
atoms/mol)
From the information given:
A = 180.9 g/mol
ρ = 16.6 g/cm^3
Since the crystal structure is BCC, n, the number of atoms per unit cell, is 2.
We can use the theoretical density ρ to find the radio <em>R</em> as follows:
Solving for <em>R</em>
![\rho=\frac{nA}{(\frac{64\sqrt{3}R^3}{9})N_{a}}\\\frac{64\sqrt{3}R^3}{9}=\frac{nA}{\rho N_{a}}\\R^3=\frac{nA}{\rho N_{a}}\cdot \frac{1}{\frac{64\sqrt{3}}{9}} \\R=\sqrt[3]{\frac{nA}{\rho N_{a}}\cdot \frac{1}{\frac{64\sqrt{3}}{9}}}](https://tex.z-dn.net/?f=%5Crho%3D%5Cfrac%7BnA%7D%7B%28%5Cfrac%7B64%5Csqrt%7B3%7DR%5E3%7D%7B9%7D%29N_%7Ba%7D%7D%5C%5C%5Cfrac%7B64%5Csqrt%7B3%7DR%5E3%7D%7B9%7D%3D%5Cfrac%7BnA%7D%7B%5Crho%20N_%7Ba%7D%7D%5C%5CR%5E3%3D%5Cfrac%7BnA%7D%7B%5Crho%20N_%7Ba%7D%7D%5Ccdot%20%5Cfrac%7B1%7D%7B%5Cfrac%7B64%5Csqrt%7B3%7D%7D%7B9%7D%7D%20%5C%5CR%3D%5Csqrt%5B3%5D%7B%5Cfrac%7BnA%7D%7B%5Crho%20N_%7Ba%7D%7D%5Ccdot%20%5Cfrac%7B1%7D%7B%5Cfrac%7B64%5Csqrt%7B3%7D%7D%7B9%7D%7D%7D)
Substitution for the various parameters into above equation yields
![R=\sqrt[3]{\frac{2\cdot 180.9}{16.6\cdot 6.023 \times 10^{23}}\cdot \frac{1}{\frac{64\sqrt{3}}{9}}}\\R = 1.43 \times 10^{-8} \:cm = 0.143 \:nm](https://tex.z-dn.net/?f=R%3D%5Csqrt%5B3%5D%7B%5Cfrac%7B2%5Ccdot%20180.9%7D%7B16.6%5Ccdot%206.023%20%5Ctimes%2010%5E%7B23%7D%7D%5Ccdot%20%5Cfrac%7B1%7D%7B%5Cfrac%7B64%5Csqrt%7B3%7D%7D%7B9%7D%7D%7D%5C%5CR%20%3D%201.43%20%5Ctimes%2010%5E%7B-8%7D%20%5C%3Acm%20%3D%200.143%20%5C%3Anm)
Answer:
37.1g are produced
Explanation:
The combustion of C₈H₁₈ is:
C₈H₁₈ + 25/2O₂ → 8CO₂ + 9H₂O
<em>Where 1 mole of C₈H₁₈ produce 8 moles of CO₂</em>
<em />
To find the mass of CO₂ that is produced we need to convert the mass of C₈H₁₈ with molar mass. Then, with the chemical equation, we can find the moles of CO₂ and its mass, as follows:
<em>Moles C₈H₁₈ -Molar mass: 114.2g/mol-</em>
12g C₈H₁₈ * (1mol / 114.2g) = 0.105 moles of C₈H₁₈
<em>Moles CO₂:</em>
As 1 mole of C₈H₁₈ produce 8 moles of CO₂, 0.105 moles of C₈H₁₈ produce:
0.105 moles of C₈H₁₈ * (8moles CO₂ / 1mole C₈H₁₈) = 0.84 moles of CO₂
<em>Mass CO₂ -Molar mass: 44.01g/mol-:</em>
0.84 moles of CO₂ * (44.01g / mol) = 37.0g of CO₂ ≈
<h3>37.1g are produced</h3>
