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denpristay [2]
2 years ago
6

Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas well

s. In the first step of this synthesis, called Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 450 liters per second of dioxygen are consumed when the reaction is run at 264 degrees Celsius and 0.48 atm.
Required:
Calculate the rate at which sulfur dioxide is being produced. Give the answer in kg per second.
Chemistry
1 answer:
galben [10]2 years ago
3 0

Answer:

0.21\ \text{kg/s}

Explanation:

P = Pressure = 0.48\ \text{atm}=0.48\times 101325\ \text{Pa}

V = Volume = 450\ \text{L/s}=450\times 10^{-3}\ \text{m}^3/\text{s}

R = Gas constant = 8.314\ \text{J/mol K}

T = Temperature = (264+273.15)\ \text{K}

The reaction is

2H_2S+3O_2\rightarrow 2SO_2+2H_2O

From ideal gas equation we have

PV=nRT\\\Rightarrow n=\dfrac{PV}{RT}\\\Rightarrow n=\dfrac{0.48\times101325\times 450\times 10^{-3}}{8.314\times (264+273.15)}\\\Rightarrow n=4.9\ \text{mol}

Moles of SO_2 produced is

\dfrac{2}{3}\times 4.9=3.267\ \text{moles}

Molar mass of SO_2 = 64.066 g/mol

Production rate is

3.267\times 64.066=209.3\ \text{g/s}=0.21\ \text{kg/s}

The rate at which sulfur dioxide is being produced 0.21\ \text{kg/s}.

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