Molar mass is 56.02 grams
D(Cr) = 8,96 g/cm3
<span>M(Cr) = 63,546 g/mol </span>
<span>In a cell face centred cubic, there are 4 atoms of Cur . . . ! </span>
<span>n(Cr in 1 cm3) = m(Cu) / M(Cr) </span>
<span>n(Cr in 1 cm3) = 8,96 / 63,546 </span>
<span>n(Cr in 1 cm3) = 0,141 mol of Cr </span>
<span>Avogadro's number is : NA = 6,02•10^23 mol^-1 </span>
<span>N(Cr) = n(Cu) x NA </span>
<span>N(Cr) = 0,141 x 6,02•10^23 </span>
<span>N(Cr) = 8,488•10^22 atoms of Cr </span>
<span>N(cell) = N(Cu) / 4 </span>
<span>N(cell) = 8,488•10^22 / 4 </span>
<span>N(cell) = 2,122•10^22 cells in 1 cm3</span>
The uses of nitrogen is that it helps eliminate the toxic chemicals in the air.
Answer:
0.482 ×10²³ molecules
Explanation:
Given data:
Volume of gas = 2.5 L
Temperature of gas = 50°C (50+273 = 323 k)
Pressure of gas = 650 mmHg (650/760 =0.86 atm)
Molecules of N₂= ?
Solution:
PV= nRT
n = PV/RT
n = 0.86 atm × 2.5 L /0.0821 atm. mol⁻¹. k⁻¹. L × 323 k
n = 2.15 atm. L /26.52 atm. mol⁻¹.L
n = 0.08 mol
Number of moles of N₂ are 0.08 mol.
Number of molecules:
one mole = 6.022 ×10²³ molecules
0.08×6.022 ×10²³ = 0.482 ×10²³ molecules
Answe
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Explanation:
We use the equation:
Mass = Number of moles * Molecular or atomic mass
Since the number of moles is 1 ("one mole of carbon-12 atoms") and the atomic mass of carbon-12 atoms is 12, hence the mass would be 12 grams. Note that the unit grams (g) is used here, as it is the SI unit for mass measurement.
Number of particles in 1 mole = 6.023 × 1023
Mass of 1 electron = 9.10938 × 10-28 gm
Mass of 1 mole of electrons = 6.023 × 1023 × 9.10938 × 10-28 = 5.486 × 10 -4
Mass of 1 proton = 1.67262 × 10 -24 gm
Mass of 1 mole of protons = 6.023 × 1023 × 1.67262 × 10 -24 gm = 1.007 gm
Mass of 1 neutron = 1.67493 × 10-24 gm
Mass of 1 mole of neutron = 1.67493 × 10-24 × 6.023 × 1023 = 1.008 gm