|Ch.1 - Intro to General Chemistry||2hrs & 53mins||0% complete||WorksheetStart|
|Ch.2 - Atoms & Elements||2hrs & 49mins||0% complete||WorksheetStart|
|Ch.3 - Chemical Reactions||3hrs & 25mins||0% complete||WorksheetStart|
|BONUS: Lab Techniques and Procedures||1hr & 38mins||0% complete||WorksheetStart|
|BONUS: Mathematical Operations and Functions||47mins||0% complete||WorksheetStart|
|Ch.4 - Chemical Quantities & Aqueous Reactions||3hrs & 55mins||0% complete||WorksheetStart|
|Ch.5 - Gases||3hrs & 47mins||0% complete||WorksheetStart|
|Ch.6 - Thermochemistry||2hrs & 28mins||0% complete||WorksheetStart|
|Ch.7 - Quantum Mechanics||2hrs & 35mins||0% complete||WorksheetStart|
|Ch.8 - Periodic Properties of the Elements||1hr & 57mins||0% complete||WorksheetStart|
|Ch.9 - Bonding & Molecular Structure||2hrs & 5mins||0% complete||WorksheetStart|
|Ch.10 - Molecular Shapes & Valence Bond Theory||1hr & 31mins||0% complete||WorksheetStart|
|Ch.11 - Liquids, Solids & Intermolecular Forces||3hrs & 40mins||0% complete||WorksheetStart|
|Ch.12 - Solutions||2hrs & 17mins||0% complete||WorksheetStart|
|Ch.13 - Chemical Kinetics||2hrs & 22mins||0% complete||WorksheetStart|
|Ch.14 - Chemical Equilibrium||2hrs & 26mins||0% complete||WorksheetStart|
|Ch.15 - Acid and Base Equilibrium||4hrs & 42mins||0% complete||WorksheetStart|
|Ch.16 - Aqueous Equilibrium||3hrs & 48mins||0% complete||WorksheetStart|
|Ch. 17 - Chemical Thermodynamics||1hr & 44mins||0% complete||WorksheetStart|
|Ch.18 - Electrochemistry||2hrs & 58mins||0% complete||WorksheetStart|
|Ch.19 - Nuclear Chemistry||1hr & 33mins||0% complete||WorksheetStart|
|Ch.20 - Organic Chemistry||3hrs||0% complete||WorksheetStart|
|Ch.22 - Chemistry of the Nonmetals||2hrs & 1min||0% complete||WorksheetStart|
|Ch.23 - Transition Metals and Coordination Compounds||1hr & 54mins||0% complete||WorksheetStart|
|Rate of Reaction||11 mins||0 completed|
|Average Rate of Reaction||18 mins||0 completed|
|Arrhenius Equation||16 mins||0 completed|
|Rate Law||38 mins||0 completed|
|Integrated Rate Law||52 mins||0 completed|
|Collision Theory||9 mins||0 completed|
|Instantaneous Rate of Change|
|Identifying Reaction Order|
Phosphine, PH3(g), decomposes according to the equation
4PH3(g) → P4(g) + 6H2 (g)
The kinetics of the decomposition of phosphine at 950 K was followed by measuring the total pressure in the system as a function of time. The data to the right were obtained in a run where the reaction chamber contained only pure phosphine at the start of the reaction. Choose the rate law that describes this reaction.
Calculate the value of the rate constant and choose the correct units.
We are asked to determine the Rate Law that describes the decomposition of Phosphine, given the temperature and the total system pressure as a function of time.
The chemical equation is:
4PH3(g) → P4(g) + 6H2(g)
Recall that the rate of reaction is the change in pressure (in this case) of a reactant for every change in time. Since we are given with the Total pressure of the system and we are only concerned with the reactant, we need to first identify the Pressure of PH3 for every given time.
At t=0, there was only PH3, therefore:
At t=40 min, we need to use the ICF chart to determine the pressure of PH3.
4PH3(g) → P4(g) + 6H2(g)
At t=40 min, total system pressure is 151 torr, therefore,
x = 17
Therefore, pressure of PH3 at t=40 is:
At t=40 min, pressure of PH3 is 32 torr.
At t=80 min, total system pressure is 168 torr, therefore,
x = 22.7
Therefore, pressure of PH3 at t=80 is:
At t=80 min, pressure of PH3 is 9.2 torr.
At t=100 min, total system pressure is 171 torr, therefore,
x = 23.7
Therefore, pressure of PH3 at t=100 is:
At t=100 min, pressure of PH3 is 5.2 torr.
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