It is a hot day in july. the temp in the morning is 5 celcius and the pressure indicator on the tak of nitrogen measures 861mmhg. durin the hottes part of the day the temp reaches a high of 28 celcius. what is the new pressure readin on the indicator?

Explanation:

The volume and amount are constant, so we can use Gay-Lussac’s Law:

At constant volume, the pressure exerted by a gas is directly proportional to its temperature.

Data:

p₁ = 861 mmHg; T₁ =   5 °C

p₂ = ?;                T₂ = 28 °C

Calculations:

(a) Convert the temperatures to kelvins

T₁ = (   5 + 273.15) K = 278.15 K

T₂ = (28 + 273.15) K = 301.15 K

(b) Calculate the pressure

idk i’m struggling too

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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