. On heating under suitable conditions, 1 liter of a monoatomic gas X combines with 1 .5litres of oxygen forming an oxide.
What is the formular of the oxide?
So the oxide is X1O1.5 or in small whole numbers is X2O3.
Well, well, well, if it isn't the chemistry detective! Let's crack this case, shall we?
Now, we know we're dealing with a monoatomic gas X. So, this means that X is an element composed of single atoms. Exciting stuff!
When 1 liter of X combines with 1.5 liters of oxygen, we need to find out the ratio to determine the formula of the oxide. But hold on a second, we have a little problem here! We can't directly compare liters because gases at the same temperature and pressure occupy molar volumes.
So, we need to convert those pesky volumes into moles using the ideal gas law (PV = nRT), assuming constant temperature and pressure. Once we have moles of each substance, we can find the ratio.
Be careful not to clown around with this calculation! It's important to have accurate figures to get the right answer. So, grab a calculator and get crunching!
Once you have the ratio, you'll be able to determine the formula of the oxide. Case closed, chemistry detective!
To determine the formula of the oxide formed when 1 liter of monoatomic gas X combines with 1.5 liters of oxygen, we need to use the concept of combining volumes of gases.
According to Avogadro's law, equal volumes of gases at the same temperature and pressure contain an equal number of molecules. Therefore, the ratio between the volumes of reacting gases gives us the ratio of the number of molecules.
From the given information, we have:
Volume of gas X (V1) = 1 liter
Volume of oxygen (V2) = 1.5 liters
To find the ratio, we can divide the volumes:
V1/V2 = 1/1.5 = 2/3
The ratio of volumes is 2:3.
Since the gas X is monoatomic, it can form only one-to-one ratio compounds with other elements. Therefore, the formula of the oxide will be determined based on this ratio.
Since the ratio of volumes is 2:3, the formula of the oxide is X2O3.
To determine the formula of the oxide formed when 1 liter of monoatomic gas X combines with 1.5 liters of oxygen, we need to consider the mole ratios of the reactants.
1 liter of gas X reacts with 1.5 liters of oxygen. However, since gases expand to fill their containers, the volumes of gases are not directly proportional to the amount of substance (moles) involved in the reaction. Therefore, we need to convert the volumes of gases to moles.
To convert the volume of a gas to moles, we use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. However, since the conditions are not specified, we will assume the temperature and pressure are constant.
Given that 1 liter of gas X combines with 1.5 liters of oxygen, we can assume they react in a 1:1 ratio. This means that for every 1 mole of gas X, 1 mole of oxygen is required to form the oxide.
Therefore, the formula of the oxide formed will depend on the valence of gas X. If gas X is a monovalent element (valence of 1), the formula of the oxide would be XO. If gas X is a divalent element (valence of 2), the formula would be XO2. And so on, depending on the valence of gas X.
Without further information about the element X or its valence, it is not possible to determine the specific formula of the oxide.