What is the theoretical yield of ammonia that can be obtained from the reaction of 17.1 g of H2 and excess N2?

1 answer:

6 0

The theoretical yield is the yield after a certain reaction occurs. So if you are given 17.1 g of H2 and an excess of N2, you should know the balanced equation.

N2 + 3H2 → 2NH3

Molar mass of H2 = 2.02 g/mol

Molar mass of NH3 = 17 g/mol

(17.1 g of H2)(1 mol H2/2.02g H2)(2 mol NH3/3mol H2)(17g NH3/1mol NH3) = 95.94g NH3

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An Sulfur tetrafluoride gas is collected at 23.0 °C in an evacuated flask with a measured volume of 20.0 L. When all the gas has

Jlenok [28]

mass = 20.48 g

moles=0.1895

<h3>Further explanation</h3>

In general, the gas equation can be written

where

P = pressure, atm

V = volume, liter

n = number of moles

R = gas constant = 0.08205 L.atm / mol K

T = temperature, Kelvin

P=0.23 atm

V=20 L

T=23+273=296 K

$\tt n=\dfrac{PV}{RT}=\dfrac{0.23\times 20}{0.082\times 296}=0.1895$

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$\tt 0.1895\times 108,07 g/mol=20.48~g$

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(If you mean by a gas of some sort)

4 0

3 years ago

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Be sure to answer all parts. what are the concentrations of hso4−, so42−, and h in a 0. 31 m khso4 solution? (hint: h2so4 is a s

disa [49]

At equilibrium the concentrations of:

[HSO₄⁻] = 0.10 M;

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[H⁺] = 0.037 M;

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HSO₄⁻ will not gain H⁺ to produce H₂SO₄ since H₂SO₄ is a strong acid. HSO₄⁻ may act as an acid and lose H⁺ to form SO₄²⁻. Let the final H⁺ concentration be x M. Construct a RICE table for the dissociation of HSO₄²⁻.

R $HSO_4^-$ ⇄ $H^+ + SO_4^2^-$