AND the reaction rate of one from that of another Most of the sulfur used in the

Question

AND the reaction rate of one from that of another Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the 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 956. liters per second of dioxygen are consumed when the reaction is run at 279·°C and 0.75 atin. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. re to search

Explanation / Answer

V = 956 L/s of O2

T = 279°C = 552 K; P = 0.75 atm

change to mol via ideal gas law

PV = nRT

n = PV/(RT) = (0.75 )(956 )/(0.082*552 ) = 15.8404 mol of O2 per second

relate to:

H2S(g) + 3/2O2(g) = SO2(g) + H2O(g)

1.5 mol of O2 = 1 mol of SO2

15.8404 mol --> 15.8404 /1.5 = 10.560 mol of SO2

mass = mol*MW = 10.560*64= 675.84 g of SO2 per second

SO2 Rate = 0.6758 kg of SO2/s

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