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Calculate the density of silver which cr...

Calculate the density of silver which crystallizes in face- centred cubic form. The distance between nearest metal atoms is 287 pm (Molar mass of `Ag = 107.87 g mol^(-1) , N_A = 6.022 xx 10^(23) mol^(-1)`).

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To calculate the density of silver (Ag) which crystallizes in a face-centered cubic (FCC) structure, we can follow these steps: ### Step 1: Understand the relationship between the edge length (A) and the nearest neighbor distance (d). In an FCC structure, the relationship between the edge length (A) and the nearest neighbor distance (d) is given by: \[ d = \frac{A}{\sqrt{2}} \] Given that the nearest metal atom distance \( d \) is 287 pm, we can rearrange this formula to find A: \[ A = d \cdot \sqrt{2} \] ...
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Calculate the density of silver which crystallises in face-centred cubic from. The distance between nearest metal atoms is 287 pm (Molar mass of Ag = 107.87gmol^(-1),(N_(0)=6.022xx10^(23)mol^(-1)) .

Niobium crystallizes in body centred cubic structure. If its density is 8.55 g cm^(-3) , calculate the atomic radius of niobium. (Atomic mass of Nb = 93u , N_A = 6.02 xx 10^(23) mol^(-1) )

Knowledge Check

  • The number of atoms in 0.1 mole of a triatomic gas is (N_(A) = 6.02 xx 10^(23) "mol"^(-1))

    A
    `6.026 xx 10^(22)`
    B
    `1.806 xx 10^(23)`
    C
    `3.600 xx 10^(23)`
    D
    `1.800 xx 10^(22)`

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