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How do you calculate equivalent weight of oxide?
To calculate the equivalent weight of an oxide, you first determine its molecular weight. Then you look at how many oxygen atoms are present in the formula of the oxide and divide the molecular weight by that number of oxygen atoms. This result is the equivalent weight of the oxide.
How do you calculate equivalent weight of anhydrous citric acid?
How do you calculate equivalent weight of anhydrous citric acid?Read more: How_do_you_calculate_equivalent_weight_of_anhydrous_citric_acid
What is the method to calculate the mass in grams of each sample?
To calculate the mass in grams of each sample, you can use a balance or scale to measure the weight of the sample. The weight measured in grams is equivalent to the mass of the sample.
How many moles is 1.50 X1023 molecules of NH3?
2.49x10-1mol NH3Source: e2020
What is can the mass NH3 made if they give you the gram?
To find the mass of NH3 produced, first calculate the number of moles of NH3 using the given mass and the molar mass of NH3. Then, use the relationship between moles and mass (mass = moles x molar mass) to find the mass of NH3.
What is equivalent weight of NH3?
17
What is the equivalent weight of NH3 in Haber's process and how?
In Haber’s process, the equivalent weight of ammonia (NH3) is calculated based on its molar mass and the number of moles of hydrogen ions (H⁺) it can donate or accept. The molar mass of NH3 is approximately 17 g/mol. Since one mole of NH3 can donate one mole of H⁺, its equivalent weight is also 17 g. Thus, the equivalent weight of NH3 in the context of Haber’s process is 17 g/equiv.
The molarity of a 5 percent solution of NH3 in water?
The molarity of a 5% solution of NH3 in water depends on the density and molecular weight of NH3. Without this information, it is not possible to calculate the molarity.
How do you calculate equivalent weight of oxide?
To calculate the equivalent weight of an oxide, you first determine its molecular weight. Then you look at how many oxygen atoms are present in the formula of the oxide and divide the molecular weight by that number of oxygen atoms. This result is the equivalent weight of the oxide.
How do you calculate equivalent weight of anhydrous citric acid?
How do you calculate equivalent weight of anhydrous citric acid?Read more: How_do_you_calculate_equivalent_weight_of_anhydrous_citric_acid
For a solution that is 0.162 m NH3 and 0.110 m NH4 cl calculate OH?
To calculate the hydroxide ion concentration in the solution, first calculate the ammonia concentration based on the NH3 concentration (NH3 is a weak base that accepts a proton to form NH4 + OH-). Then, use the Kb value for NH3 to find the OH- concentration from NH3's hydrolysis reaction. Finally, don't forget to consider the contribution of OH- from the dissociation of NH4OH for the total OH- concentration.
If you have 14 grams of N2 how much NH3 can you make?
First you have to balance the equation N2 + H2 ---> NH3 N2 +3H2 ---> 2NH3 Then you have to use the Molecular Weight and number of mols required for complete reaction of each one to go from 14g N2 + xg of H2 to get the final result.
What is the method to calculate the mass in grams of each sample?
To calculate the mass in grams of each sample, you can use a balance or scale to measure the weight of the sample. The weight measured in grams is equivalent to the mass of the sample.
How many moles is 1.50 X1023 molecules of NH3?
2.49x10-1mol NH3Source: e2020
What mass of NH3 can be made from 35.0g of N2?
Relation of mols : N2 + 4H2 → 2NH4This means : 1 mol of molecular nitrogen will give you 2 mols of ammonia.Atomic weight : N; 14.0067, H; 1.00797Molecular weight : N2 ; 28.0134 g/mol, NH4; 18.03858 g/molFrom mol relation, the weight relation is: 28.0134 g of N2 give 36.00772 g of NH4So 35.0 g of N2 will give you: 36.00772 g x 35.0 g / 28.0134 g ~ 45.0 g of NH4
How do you calculate the equivalent weight of compound?
the sum of the atomic weights for all the atoms in the formula
How do you calculate gram equivalent weight.?
Gram equivalent weight is calculated by dividing the molar mass of the compound by the number of equivalents of the species involved in the reaction. It is a measure of the mass of a substance that provides one equivalent of the species of interest in a chemical reaction.
