What are 3 types of mutations

Chemistry

2 answers:

mote1985 [20]2 years ago

6 0

1- Base substitutions.

2- Deletions.

3- Insertions.

STALIN [3.7K]2 years ago

5 0

If u take a close look at the teenage mutant ninja turtles you will see

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aqueous lithium hydroxide solution is used to purify air (remove co2) in spacecrafts and submarines. the pressure of carbon diox

oksano4ka [1.4K]

The mass of the water is 1580 g.

<h3>What is the amount of water formed?</h3>

We know that the ideal gas equation can be used to obtain the number of moles of the gas. We have been told that the pressure of the gas reduced from 7.9 x 10-3 atm to 1.2 x 10-4 atm. The change in pressure can be used obtain the number of moles.

Change in pressure = 7.9 x 10-3 - 1.2 x 10-4 = 7.78 * 10^-3 atm

Using;

PV = nRT

n = PV/RT

n = 7.78 * 10^-3 atm * 2.4 x10^5 l/0.082 * (39 + 273)

n = 85 moles

Since 1 mole of carbon dioxide produces 1 mole of water

85 moles of carbon dioxide produces 85 mole of water

Mass of water produced = 85 mole * 18 g/mol

= 1580 g

Learn more about ideal gas equation:brainly.com/question/4147359

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6 0

8 months ago

If you are given an ideal gas with pressure (p)259,392.00 pa and temperature (T)=200°c of 1 mole Argon gas in a volume 8.8dm3,ca

GuDViN [60]

Answer: $R=4.82436 \frac{Pa. m^{3}}{mol. K}$

Explanation:

The Ideal Gas equation is:

$P.V=n.R.T$ (1)

Where:

$P$ is the pressure of the gas

$n$ the number of moles of gas

$R=8.3144598 \frac{Pa. m^{3}}{mol. K}$ is the gas constant

$T$ is the absolute temperature of the gas in Kelvin.

$V$ is the volume

It is important to note that the behavior of a real gas is far from that of an ideal gas, taking into account that <u>an ideal gas is a single hypothetical gas</u>. However, under specific conditions of standard temperature and pressure (T=0\°C=273.15 K and P=1 atm=101,3 kPa) one mole of real gas (especially in noble gases such as Argon) will behave like an ideal gas and the constant R will be $8.3144598 \frac{Pa. m^{3}}{mol. K}$ .

However, in this case we are not working with standard temperature and pressure, therefore, even if we are working with Argon, the value of R will be far from the constant of the ideal gases.

Having this clarified, let's isolate $R$ from (1):