Which one of the following changes would cause the number of collisions between

Question

Which one of the following changes would cause the number of collisions between molecules of gas to DECREASE? Mark all correct choices. (a) Increasing the gas pressure while keeping temperature unchanged (b) Decreasing the gas volume while keeping its amount unchanged (c) Increasing the gas volume while keeping its amount unchanged (d) Decreasing the molecular weight of gas while keeping temperature unchanged (e) Increasing the molecular weight of gas while keeping temperature unchanged 9. 10. Initial rates shown below were measured for the following hypothetical reaction: 2A(g) + B(g) + 2C(g)-> D(g) + E(g) What is the correct rate law for this reaction? Trial [AL IB ICl 1 0.225 0.150 0.350 0.0217 2 0.320 0.150 0.350 0.0439 3 0.225 0.250 0.350 0.0362 4 0.225 0.150 0.600 0.01270

Explanation / Answer

Ans 9 The correct choices are : c) Increasing the gas volume while keeping its amount unchanged ; e) Increasing the molecular weight of gas while keeping the temperature unchanged.

The number of collisions of gas particles depend on variety of different factors : pressure , volume , molecular weight to name a few. When the pressure is decreased or the volume is increased , the frequency of and number of collisons of gas molecules decreases. When the molecular weight of the gas is increased , its average kinetic energy decreases , which eventually decreases the number of collisions too.

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