What is the major use of carbon monoxide

Chemistry

1 answer:

Dmitry [639]2 years ago

8 0

Answer:

Carbon monoxide is a very important industrial compound. In the form of producer gas or water gas.

hope ths help and if you want more information go to this website: science.jrank.org

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The reduced vapor pressure at high altitudes causes a liquid to boil at a temperature.

irinina [24]

At higher altitudes (and thus lower atmospheric pressures), water boils at a lower temperature. This is because the lack of vapor pressure at that altitude doesn't constrain the speed of the molecules with barometric pressure. Therefore, the water begins boiling at a lower temperature. This is often a disadvantage because even if the water is boiling, it won't be hot enough for meals (which is why heat and temperature are distinct). That's why we have pressure cookers, which manage to keep a stable boiling point.
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3 years ago

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How can a sea cave become a sea arch?

navik [9.2K]

Erosion. The waves breaking on the cave and washing up on it will eventually start breaking down the rocks

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3 years ago

How many moles of a gas would occupy 22.4 Liters at 273 K and 1 atm?

Molodets [167]

Answer:

1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm

Explanation:

An ideal gas is a set of atoms or molecules that move freely without interactions. The pressure exerted by the gas is due to the collisions of the molecules with the walls of the container. The ideal gas behavior is at low pressures, that is, at the limit of zero density. At high pressures the molecules interact and intermolecular forces cause the gas to deviate from ideality.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

P= 1 atm
V= 22.4 L
n= ?
R= 0.082 $\frac{atm*L}{mol*K}$
T=273 K

Reemplacing:

1 atm* 22.4 L= n* 0.082 $\frac{atm*L}{mol*K}$ *273 K

Solving:

$n=\frac{1 atm* 22.4 L}{0.082 \frac{atm*L}{mol*K} *273 K}$

n= 1 mol

Another way to get the same result is by taking the STP conditions into account.

The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C (or 273 K) are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.

1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm

4 0

2 years ago

A gas occupies the volume of 215ml at 15C and 86.4kPa?

kherson [118]

Answer:

About 0.1738 liters

Explanation:

Using the formula PV=nRT, where p represents pressure in atmospheres, v represents volume in liters, n represents the number of moles of ideal gas, R represents the ideal gas constant, and T represents the temperature in kelvin, you can solve this problem. But first, you need to convert to the proper units. 215ml=0.215L, 86.4kPa is about 0.8527 atmospheres, and 15C is 288K. Plugging this into the equation, you get:

$0.8527\cdot 0.215=n \cdot 0.0821 \cdot 288\\n\approx 7.754 \cdot 10^{-3}$