Answer:
2.22 g/L
Explanation:
There's a relationship using the ideal gas law between molar mass and density: 
, where MM is the molar mass, d is the density, R is the gas constant, T is the temperature, and P is the pressure.
We know from the problem that MM = 32.49 g/mol, T = 458 Kelvin, and P = 2.569 atm. The gas constant, R, in terms of the units atm and Kelvin is 0.08206. Let's substitute these values into the formula:
Solve for d:
d * 0.08206 * 458 K = 32.49 * 2.569
d = (32.49 * 2.569) / (0.08206 * 458 K) ≈ 2.22 g/L
The answer is thus 2.22 g/L.
<em>~ an aesthetics lover</em>
You can find the answer on chegg.com. Hope that help :)
Answer:
La distinción entre la química teóricamente teórica y la química avanzada es la química teórica teórica que se basa en un espiritualista, potente que percibe visualmente la autenticidad, mientras que la química espera que la autenticidad sea fundamentalmente mundana. Eso engendra una tremenda distinción, y la química nunca se hubiera alejado excepcionalmente de la remota posibilidad de que se hubiera quedado con el trascendentalismo antediluviano.
Explanation:
Answer : The correct option is, (1) Gains an electron and its radius increases.
Explanation :
The given element is chlorine.
Atomic number of chlorine = '17'
The electronic configuration of chlorine is, 
Number of electrons = 17
Number of protons = 17
The electronic configuration of chloride ion is, 
Number of electrons = 18
Number of protons = 17
When the chlorine atom gains an electron to acquire a stable electronic configuration. As the electrons add in the valence shell of the chlorine, the number of electrons increases but the number of protons remains the same. So, the protons will not be able to bind the extra electron and it will remain far from the nucleus.
Answer:
31 moles
Explanation:
The balanced combustion reaction of the wax, 
is shown below as:
As seen from the reaction,
1 mole of wax, on combustion produces 31 moles of carbon dioxide, 
<u>Hence, moles of when 1 mole of wax, is burnt = 31 moles</u>
