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3 years ago

A chemist wade out 5.96 grams of barium calculate the number of moles of barium she weighed out

Chemistry

1 answer:

PilotLPTM [1.2K]3 years ago

7 0

Answer:

0.04 mol

Explanation:

Given data:

Mass of barium = 5.96 g

Moles of barium = ?

Solution:

Formula:

Number of moles = mass/molar mass

Molar mass of barium = 5.96 g/ 137.33 g/mol

Number of moles = 0.04 mol

Thus the number of moles of barium in 5.96 g are 0.04 moles. The chemist weight out the 0.04 moles .

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The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibri

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Volume of vessel = 1.00 L

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$\text{Molarity}=\frac{\text{Number of moles}}{\text{Volume of solution (in L)}}$

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The given chemical equation follows:

$NH_4Cl(s)\rightleftharpoons NH_3(g)+HCl(g)$

Initial: 0.564

At eqllm: 0.564-x x x

The expression of $K_c$ for above equation follows:

$K_c=[NH_3][HCl]$

The concentration of pure solid and pure liquid is taken as 1.

We are given:

$K_c=5.10\times 10^{-6}$

Putting values in above equation, we get:

$5.10\times 10^{-6}=x\times x\\\\x=2.26\times 10^{-3}M,-2.26\times 10^{-3}M$

Negative sign is neglected because concentration cannot be negative.

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