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Stella [2.4K]
3 years ago
7

What is the average kinetic energy of a gas at 285 kelvin? (R = 8.314 J/K-mol)

Chemistry
2 answers:
maxonik [38]3 years ago
6 0
The answer would be 3.55 x 10^3 j/mol
Svetllana [295]3 years ago
6 0

Answer:

The average KE = 312 J/mol

Explanation:

<u>Given:</u>

Temperature of the gas, T = 285 K

Gas constant, R = 8.314 J/K-mol

<u>To determine:</u>

The average kinetic energy of the gas

<u>Explanation:</u>

Based on the kinetic theory of gases, the average kinetic energy is given as:

KE = \frac{3}{2} RT\\

In this case:

KE = \frac{3}{2} *8.314\ J/K-mol * 285\ K = 312 J/mol

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4 0
2 years ago
7.) A syringe initially holds a sample of gas with a volume of 285 mL at 355 K and 1.88 atm. To
marysya [2.9K]

Answer:

T₂ = 721 k

Explanation:

Given data:

Initial volume = 285 mL

Initial pressure = 1.88 atm

Initial temperature = 355 K

Final temperature = ?

Final volume = 435 mL

Final pressure = 2.50 atm

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

P₁V₁/T₁ = P₂V₂/T₂  

T₂  =  P₂V₂ T₁  / P₁V₁

T₂ = 2.50 atm × 435 mL × 355 K / 1.88 atm × 285 mL  

T₂ = 386062.5 atm. mL. K /535.8 atm. mL

T₂ = 721 k

5 0
3 years ago
Calculate the pH for the following weak acid. A solution of HCOOH has 0.12M HCOOH at equilibrium. The Ka for HCOOH is 1.8×10−4.
Shtirlitz [24]

Answer:

the pH of HCOOH solution is 2.33

Explanation:

The ionization equation for the given acid is written as:

HCOOH\leftrightarrow H^++HCOO^-

Let's say the initial concentration of the acid is c and the change in concentration x.

Then, equilibrium concentration of acid = (c-x)

and the equilibrium concentration for each of the product would be x

Equilibrium expression for the above equation would be:

\Ka= \frac{[H^+][HCOO^-]}{[HCOOH]}

1.8*10^-^4=\frac{x^2}{c-x}

From given info, equilibrium concentration of the acid is 0.12

So, (c-x) = 0.12

hence,

1.8*10^-^4=\frac{x^2}{0.12}

Let's solve this for x. Multiply both sides by 0.12

2.16*10^-^5=x^2

taking square root to both sides:

x=0.00465

Now, we have got the concentration of [H^+] .

[H^+] = 0.00465 M

We know that, pH=-log[H^+]

pH = -log(0.00465)

pH = 2.33

Hence, the pH of HCOOH solution is 2.33.

7 0
3 years ago
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