Statement 2 is correct.
solids moving into solution is a physical change as the core structure of the molecules remain the same. evaporation of water and crystallization of salt are both physical changes as well.
The water does not change it's H2O chemical makeup because salt was dissolved into it.
Sandblasted: More smooth because all the rough edges are "blasted" away. And slightly smaller because of the loss of the edges.
Non-Sandblasted: Not smooth; rough.
The answer to this question would be liquid.
<span>Lipids with high polyunsaturated fatty acid mostly found as a liquid, but the saturated one would be solid at room temperature. A molecule with higher molecular weight will have the higher boiling point and it more likely to be solid at room temperature.
Unsaturated fat is more healthy than saturated fat and it is recommended to reduce saturated fat consumption as it was linked to many diseases.
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The molecular formula : As₄S₆
<h3>Further explanation</h3>
Given
Rate of effusion of arsenic(III) sulfide = 0.28 times the rate of effusion of Ar atoms
Required
The molecular formula
Solution
Graham's law: the rate of effusion of a gas is inversely proportional to the square root of its molar masses or
the effusion rates of two gases = the square root of the inverse of their molar masses:
or
Input the value :
1 = Arsenic(III) sulfide
2 = Ar
MM Ar = 40 g/mol
0.28 = √(40/M₁)
M₁=40 : 0.28²
M₁=510 g/mol
The empirical formula of arsenic(III) sulfide = As₂S₃
(Empirical formula)n = molecular formula
( As₂S₃)n = 510 g/mol
(246.02 g/mol)n = 510 g/mol
n = 2
So the molecular formula : As₄S₆
Answer: First, here is the balanced reaction: 2C4H10 + 13O2 ===> 8CO2 + 10H2O.
This says for every mole of butane burned 4 moles of CO2 are produced, in other words a 2:1 ratio.
Next, let's determine how many moles of butane are burned. This is obtained by
5.50 g / 58.1 g/mole = 0.0947 moles butane. As CO2 is produced in a 2:1 ratio, the # moles of CO2 produced is 2 x 0.0947 = 0.1894 moles CO2.
Now we need to figure out the volume. This depends on the temperature and pressure of the CO2 which is not given, so we will assume standard conditions: 273 K and 1 atmosphere.
We now use the ideal gas law PV = nRT, or V =nRT/P, where n is the # of moles of CO2, T the absolute temperature, R the gas constant (0.082 L-atm/mole degree), and P the pressure in atmospheres ( 1 atm).
V = 0.1894 x 0.082 x 273.0 / 1 = 4.24 Liters.
Explanation:
