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wouldn't it be more than 1 g? i say this because the first substance that the oxygen would chemically combine to would have its own mass (1g), and once the oxygen combines to it, wouldn't the mass of the oxygen and the substance also combine, forming a new mass greater than 1 g?
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When 1.326 g of a metal sulfide was roasted in air 0.824 g of oxide was formed If the oxidation number of the metal is 2 what is the molar mass of the metal?
Since the metal sulfide is being converted to metal oxide, there is an increase in mass corresponding to the oxygen atoms gained. The difference in mass is due to the oxygen incorporated from the air, allowing us to find the molar mass of the metal by calculating the moles of oxygen gained and then determining the atomic mass of the metal.
IFA metal forms two oxides the higher oxide contain 80 Metal 0.72Gm of lower oxide gave 0.8Gm of the higher oxide when oxidized show these data illustrate law of multiplication?
The law of multiplication states that when elements combine to form more than one compound, the mass of one element that combines with a fixed mass of the other element is a simple ratio of small whole numbers. In this case, the data provided show that the ratio of the masses of metal in the two oxides (0.8g / 0.72g) is a simple ratio, demonstrating the law of multiplication in action.
In which of the oxides: manganese (IV) oxide or magnesia is a greater percentage by mass of non-metal, and in which there is a greater percentage by mass of metal. Give the formulas of both oxides, write down the calculations and the answer?
ammonium carbonate
A particular element M has a heat capacity of 0.36 JgK and it forms an oxide that contains 2.9 grams of M per gram of oxygen What is the molar mass of the metal?
To find the molar mass of the metal (M), first, calculate the molar mass of the oxide. Since one gram of the oxide contains 2.9 grams of M and 1 gram of oxygen, the molar mass of the oxide is M + O = 2.9M + 16. Using the heat capacity, you can calculate the molar mass of the oxide, which in turn gives you the molar mass of the metal M.
What is the mass of 24.6 formula units of magnesium oxide?
To find the mass of 24.6 formula units of magnesium oxide, we first need to determine the molar mass of magnesium oxide. Magnesium has a molar mass of approximately 24.3 g/mol, and oxygen has a molar mass of approximately 16.0 g/mol. Therefore, the molar mass of magnesium oxide (MgO) is 24.3 + 16.0 = 40.3 g/mol. Next, we multiply the molar mass of MgO by the number of formula units (24.6) to find the total mass: 40.3 g/mol x 24.6 = 992.38 grams. Therefore, the mass of 24.6 formula units of magnesium oxide is approximately 992.38 grams.
When 1 gram of metal is oxidized what is the resulting mass?
The resulting mass is the same as the original mass, as the total mass during oxidation remains constant due to the conservation of mass principle.
Why does the mass of copper oxide not lose mass when heated?
When copper oxide is heated, it undergoes a chemical reaction that causes it to lose oxygen atoms, resulting in the formation of copper metal. The mass of the copper metal formed is equal to the mass of the original copper oxide. Therefore, the overall mass remains the same.
When 1.187 grams of metallic oxide is reduced with excess hydrogen 1.054 grams of the metal is produced What is the metallic oxide?
The molar mass of the metal can be found by taking the difference in mass before and after reduction. The difference in mass is 0.133 grams and the molar mass of the metal is determined to be 29 grams/mol, suggesting the metallic oxide is iron (III) oxide (Fe2O3).
Which of these alkaline earth metal oxides has the greatest percent by mass oxygen 1 barium oxide 2 beryllium oxide 3 calcium oxide 4 magnesium oxide 5 strontium?
2. beryllium oxide. Each oxide contains as many oxygen atoms as alkaline earth metal atoms, and beryllium has the smallest atomic weight of the alkaline earth metals. Therefore, beryllium oxygen has the greatest percentage by weight of oxygen.
If the oxide contains 22.55 percent O by mass what is the identity of the metal?
To find the identity of the metal in the oxide, we need to determine the percent composition of the metal. Since the oxide contains 22.55% oxygen by mass, the metal must make up the remaining percentage of the compound. Subtracting 22.55 from 100 gives 77.45%, which indicates the metal makes up 77.45% of the compound by mass.
A metal forms two oxidesThe higher oxide contains 80 percent metal 0.72g of lower oxide gave 0.8g of the higher oxide when oxidised Show that the data illustrates the law of multiple proportions?
In higher oxide Metal = 80% Oxygen = (100-80)% = 20% Therefore, we can say that 4 parts of metal combines with 1 part of oxygen. Now, 0.72 g of lower oxide on oxidation gives 0.8 g of higher oxide. It can be assumed that the mass percent of metal in 0.8 g is same as that of 0.72 g of lower oxide. So, Mass of metal in higher oxide = (80/100) x 0.8 g = 0.64 g If in 0.8 g of higher oxide 0.64 g is metal then mass of oxygen present in higher oxide will be (0.8 - 0.64) g = 0.16 g Since, lower oxide contains the same mass of metal as that of higher oxide, we need to calculate the mass of oxygen in lower oxide. Mass of oxygen in lower oxide = (0.72-0.64) g = 0.08 g According to Law to multiple proportions if two elements combine with each other to form two different compounds then the ratio of masses of that element which combines with the other element whose mass is fixed in both the compounds, will be in small whole numbers. Now, in the given problem the mass of metal in both the oxide is fixed so, for the data to illustrate the law of multiple proportion the ratio of mass of oxygen in both the oxides should be in whole numbers. Now, mass of oxygen in higher oxide : mass of oxygen in lower oxide = 0.16 : 0.08 = 2 : 1. Therefore, it can be said that the given data depicts law of multiple proportion.
When 1.326 g of a metal sulfide was roasted in air 0.824 g of oxide was formed If the oxidation number of the metal is 2 what is the molar mass of the metal?
Since the metal sulfide is being converted to metal oxide, there is an increase in mass corresponding to the oxygen atoms gained. The difference in mass is due to the oxygen incorporated from the air, allowing us to find the molar mass of the metal by calculating the moles of oxygen gained and then determining the atomic mass of the metal.
IFA metal forms two oxides the higher oxide contain 80 Metal 0.72Gm of lower oxide gave 0.8Gm of the higher oxide when oxidized show these data illustrate law of multiplication?
The law of multiplication states that when elements combine to form more than one compound, the mass of one element that combines with a fixed mass of the other element is a simple ratio of small whole numbers. In this case, the data provided show that the ratio of the masses of metal in the two oxides (0.8g / 0.72g) is a simple ratio, demonstrating the law of multiplication in action.
In which of the oxides: manganese (IV) oxide or magnesia is a greater percentage by mass of non-metal, and in which there is a greater percentage by mass of metal. Give the formulas of both oxides, write down the calculations and the answer?
ammonium carbonate
What is the mass for sodium oxide plus water?
The mass of sodium oxide plus water would be the sum of the masses of sodium oxide and water individually. Sodium oxide has a molar mass of 62 g/mol and water has a molar mass of 18 g/mol. By knowing the amount of each substance, you can calculate the total mass.
Why did mercuric oxide in Lavoisier reaction chamber weigh more than the mercury metal?
The air surrounding said Mercury metal was absorbed into the mercury at the higher temperatures, therefore causing the new substance--mercuric oxide--to weigh more.
When 24g of magnesium metal is heated in air 40g of magnesium oxide is produced. What mass of magnesium would be needed in order to produce 10g of magnesium oxide?
6g
