Answer:
6.
Explanation:
G, H, O, N, Na, P
There are 6 different elements listed, with O (oxygen) showing up twice.
Before we solve for the final temperature, the initial temperature should be given. Suppose this is at room temperature, 25°C. The solution is as follows.
8.8 g(1/Molar mass of benzene)(Heat of combustion of benzene) = 5,691 g water(Heat capacity of water)(Tfinal - Tinitial)
Heat from benzene = - Heat from water
8.8 g(1/78 g/mol)(-3,271 kJ/mol) = -(5,691 g)(4.816 J/g·°C)(1 kJ/1000 J)(Tfinal - 25°C)
<em>Tfinal = 38.46°C</em>
20 A
30 b
19 c
13 D
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In order to determine the number of molecules of nitrogen dioxide that are in 1.28 g of nitrogen dioxide, we first need to know these values:
Molar mass of nitrogen dioxide = 46.0055 g/mol
Avogadro's number = 6.022 x 10^23 molecules/mol
Then, we divide 1.28 g by the molar mass and multiply the resulting value to Avogadro's number:
1.28 g/ 46.0055 g/mol x 6.022 x 10^23 molecules/mol = 1.6755 x 10^22 molecules of nitrogen dioxide
Answer:Theoretical density =2.576g/cm³
Explanation:
Theoretical density p= (A×n)/Vc ×Av
A= molecular weight
n= effective number of atoms per unit cell
Vc=Volume of unit cell = a³
Av = Avogadro's constant = 6.02×10²³
Given that A= 87.2g/mol
n= 4 (For FCC crystal structure)
Vc= a³
Where a = 2R√2 and R is the atomic radius
R=0.215
a= 2 × 0.215×√2
a= 0.608nm = 0.608×10^-7 cm
Vc= (0.608×10^-7 cm)³
Vc=2.25×10^-22 cm³
P= (87.2 × 4)/
(2.25×10^-22) × (6.02×10²³)
P= 2.576g/cm³
Therefore the theoretical density of strontium is 2.576g/cm³
