If I have 2.5 moles of a gas at a pressure of 7.4 atm and volume of 8.2 liters. What is the temperature
1 answer:
Answer:
295.78K
Explanation:
For this question you can use the ideal gas law, which is
where P is pressure, V is volume, n is moles of substance, R is the ideal gas constant, and T is temperature.
We need to find temperature, so we need to rearrange the equation to solve for T
We are given n=2.5mol, P=7.4atm, and V=8.2L. We can use the gas constant R=.08206 to find the temperature in kelvin. To do so, plug all of the values into the equation (I'll be excluding units for simplicity)
The temperature is 295.78K. To find it in Celsius, subtract 273.
You might be interested in
Complete Question
The complete question is shown on the first uploaded image
Answer:
The concentration of that should used originally is
Explanation:
From the question we are told that
The necessary elementary step is
The time taken for sixth of 0.5 M of reactant to react
The time available is
The desired concentration to remain
Let Z be the reactant , Y be the first product and X the second product
Generally the elementary rate law is mathematically as
Where k is the rate constant , is the concentration of Z
From the elementary rate law we see that the reaction is second order (This because the concentration of the reactant is raised to power 2 )
For second order reaction
Where is the initial concentration of Z which a value of
From the question we are told that it take 9 hours for the concentration of the reactant to become
So
=>
For
