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3 years ago

Using the combined gas law, calculate the following. Also, what other law could you have used to solve this problem?

Chemistry

1 answer:

blsea [12.9K]3 years ago

8 0

Answer:

4.23 L

Explanation:

The question doesn't specify pressure so

i will just assume it is 1 atm. This won't affect the answer. The same result can be achieved using the combined gas law and Charle's law, so long as pressure is kept constant in the combined gas law.

Using the combined gas law

(P1 × V1)/ T1 = (P2 × V2)/T2

where

P1 = 1 atm

V1 = 4 L

T1 =293.15 K

P2 = 1 atm

V2 =?

T2=310.15 K

We can rearrange the equation to make V2 the subject

V2= (((P1 × V1)/ T1) × T2)/P2

V2 = (((1 × 4)/293.15)×310.15)/1

V2 = 4.23 L

Using Charle's law

V1/ T1 = V2/ T2

V2 = (V1/T1) × T2

V2 = (4/293.15) ×310.15

V2 =4.23L

Hopefully this is correct

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Answer:

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Explanation:

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2 years ago

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What is the half-life of a pharmaceutical if the initial dose is 500 mg and only 31 mg remains after 6 hours?

Sergeu [11.5K]

Answer:

$\large \boxed{\text{b. 1.5 h}}$

Explanation:

1. Calculate the rate constant

The integrated rate law for first order decay is

$\ln \left (\dfrac{A_{0}}{A_{t}}\right ) = kt$

where

A₀ and A_t are the amounts at t = 0 and t

k is the rate constant

$\begin{array}{rcl}\ln \left (\dfrac{500}{31}\right) & = & k \times 6\\\\\ln 16.1 & = & 6k\\2.78& =& 6k\\k & = & \dfrac{2.78}{6}\\\\& = & 0.463 \text{ h}^{-1}\\\end{array}$