How Do You Calculate the Production Rates of P4 and H2 in a Chemical Reaction?

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SUMMARY

The discussion focuses on calculating the production rates of P4 and H2 from the reaction 4PH3(g) → P4(g) + 6H2(g). In the experiment, 0.0048 mol of PH3 is consumed per second in a 2.0 L container. The production rates are derived by first converting the consumption rate to molarity (0.0024 M) and then applying stoichiometric coefficients from the balanced equation. The final rates of production for P4 and H2 are determined using these coefficients, confirming the relationship between reactants and products in a constant rate scenario.

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Could someone could help me with this reaction rate problem?
4PH3(g) ------- P4(g) + 6H2(g)
If, in a certain experiment, over a specific time period, 0.0048 mol PH3 is consumed in a 2.0 L container each second of reaction, what are the rates of production of P4 and H2 in this experiment.
I'm almost certain I have to use the coefficients in order to find the answer, but I'm having some difficulty in making any connections.
Thanks
 
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I think I finally got it, first you have to divide 2.0 into 1.0, thus making .0048 into .0024, then use a proportion with the coefficients to get the answers.
 
yeah, you're on the right track, but this is particularly easy case since you're concerned with the rate of the reaction during a time range during which the rate is constant.
 
Last edited:

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