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1 year ago

What is the mass of 0.257 mol of calcium nitrate?

Chemistry

1 answer:

poizon [28]1 year ago

4 0

Answer: 42.14 g

Explanation: calcium nitrate - $Ca(NO_{3} )_{2}$

, the molar mass of calcium nitrate = 164 g

<h3> formula used = $given mass/molar mass$ = no of moles </h3>

mass required = $0.257*164$

= $42.14$ g

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In a reaction vessel, 17.6 g of solid chromium(III) oxide, Cr2O3, was allowed to react with excess carbon tetrachloride in the f

notsponge [240]

Answer:

72.53% is the yield of CrCl3

Explanation:

Given

Reaction:

Cr2O3(s) + 3 CCl4(l) → 2 CrCl3(s) + 3 COCl2(aq)

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To Find:

% yields of the reaction

Also given

Molar mass of CrCl3 = 158.35g/mol

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By the stoichiometry of the reaction

1 mole of Cr2O3 gives 2 moles of CrCl3

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3 years ago

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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<u>Answer:</u> The equilibrium concentration of HCl is $2.26\times 10^{-3}M$

<u>Explanation:</u>

We are given:

Moles of $NH_4Cl(s)$ = 0.564 moles

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Molarity is calculated by using the equation:

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Molarity of $NH_4Cl=\frac{0.564}{1}=0.564M$

The given chemical equation follows:

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<u>At eqllm:</u> 0.564-x x x

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$K_c=[NH_3][HCl]$

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.

So, $[HCl]=2.26\times 10^{-3}M$

Hence, the equilibrium concentration of HCl is $2.26\times 10^{-3}M$

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