604 g
Ammonium chlorate is an inorganic compound with the formula NH4ClO3. ---- It is obtained by neutralizing chloric acid with either ammonia or ammonium carbonate, or by precipitating barium, strontium or calcium chlorates with ammonium carbonate or ammonium sulfate, producing the respective carbonate or sulfate precipitate and an ammonium chlorate solution. Ammonium chlorate crystallizes in small needles, readily soluble in water. On heating, ammonium chlorate decomposes at about 102 °C, with liberation of nitrogen, chlorine and oxygen. It is soluble in dilute aqueous alcohol, but insoluble in strong alcohol. This compound is a strong oxidizer and should never be stored with flammable materials. Ammonium chlorate is a very unstable oxidizer and will decompose, sometimes violently, at room temperature. It will explode when exposed to sunlight for a few minutes. Even solutions are known to be unstable. Because of the dangerous nature of this salt it should only be kept in solution when needed, and never be allowed to crystallize.
To make 3 litres of 5mM Ammonium acetate solution, you would need to calculate the amount of Ammonium acetate needed based on its molecular weight. Once you have determined the mass needed, dissolve it in sufficient water to make the final volume of 3 litres. Keep in mind to use a balance to measure out accurate amounts of the compound for precise results.
To make a 0.25M solution of ammonium sulfate at a concentration of 6M, you would need to dilute the 6M solution. Assuming you have 1 liter of the 6M solution, you can calculate the volume needed for dilution using the formula: (C1V1 = C2V2), where C1 = 6M, V1 = volume of the 6M solution (in liters), C2 = 0.25M, and V2 = total volume of the diluted solution (in liters). Once you have the volume, you can convert it to grams using the molar mass of ammonium sulfate.
To test the percent purity of potassium chlorate, you can perform a titration with a known concentration of a reducing agent, such as iron(II) sulfate, and determine the amount of reducing agent needed to completely react with the potassium chlorate. From the titration results, you can calculate the purity of the potassium chlorate by comparing the actual amount of potassium chlorate in the sample to the theoretical amount that should be present based on the reaction stoichiometry.
To make a 0.1N solution of ferrous ammonium sulfate, you first need to calculate the molecular weight of the compound. Then, you can dissolve the calculated amount of ferrous ammonium sulfate in the appropriate volume of water to prepare the desired concentration. Finally, make adjustments to the pH if needed.
(NH4)+ is Ammonium ion and (CLO3)- is chlorate ion; therefore, the name of the substance would be: Ammonium Chlorate. It is an inorganic compound. It crystallizes in small needles, readily soluble in water. It decomposes at about 102 °C, with liberation of nitrogen, chlorine and oxygen. It is soluble in dilute aqueous alcohol, but insoluble in strong alcohol. Ammonium Chlorate is obtained by neutralizing chloric acid with either ammonia or ammonium carbonate, or by precipitating barium, strontium or calcium chlorates with ammonium carbonate or ammonium sulfate, producing the respective carbonate or sulfate precipitate and an ammonium chlorate solution. Ammonium chlorate is a strong oxidizer and should never be stored with flammable materials. It is very unstable, and will decompose, sometimes violently, at room temperature. This results from the mixture of the reducing ammonium cation and the oxidizing chlorate anion. Even solutions are known to be unstable. Because of the dangerous nature of this salt it should only be kept in solution when needed, and never be allowed to crystallize.
Ammonium chlorate is an inorganic compound with the formula NH4ClO3. ---- It is obtained by neutralizing chloric acid with either ammonia or ammonium carbonate, or by precipitating barium, strontium or calcium chlorates with ammonium carbonate or ammonium sulfate, producing the respective carbonate or sulfate precipitate and an ammonium chlorate solution. Ammonium chlorate crystallizes in small needles, readily soluble in water. On heating, ammonium chlorate decomposes at about 102 °C, with liberation of nitrogen, chlorine and oxygen. It is soluble in dilute aqueous alcohol, but insoluble in strong alcohol. This compound is a strong oxidizer and should never be stored with flammable materials. Ammonium chlorate is a very unstable oxidizer and will decompose, sometimes violently, at room temperature. It will explode when exposed to sunlight for a few minutes. Even solutions are known to be unstable. Because of the dangerous nature of this salt it should only be kept in solution when needed, and never be allowed to crystallize.
To find the grams of potassium chlorate needed, you would first calculate the moles of potassium chlorate using the molarity and volume provided. Then, use the molar mass of potassium chlorate to convert moles to grams. So, the calculation would be: moles = Molarity x Volume (in liters), and then grams = moles x molar mass of potassium chlorate.
The answer is 1 mole potassium chlorate.
To find the amount of ammonium carbonate needed, use the formula: grams = moles * molar mass. First, calculate moles using the given volume and molarity: moles = volume (L) * molarity (mol/L). Then, multiply the moles by the molar mass of ammonium carbonate (96.09 g/mol) to find the grams needed.
For the decomposition of potassium chlorate, the molar ratio between potassium chlorate (KClO3) and oxygen (O2) is 2:3. Therefore, to produce 15 moles of oxygen, 10 moles of potassium chlorate are needed. (15 moles O2) x (2 moles KClO3 / 3 moles O2) = 10 moles KClO3.
Four moles of potassium chlorate are needed.
To make 3 litres of 5mM Ammonium acetate solution, you would need to calculate the amount of Ammonium acetate needed based on its molecular weight. Once you have determined the mass needed, dissolve it in sufficient water to make the final volume of 3 litres. Keep in mind to use a balance to measure out accurate amounts of the compound for precise results.
To find the amount of solution, we first determine the number of moles in 16.9 g of ammonium acetate. Then, we use the molarity to calculate the volume of the solution needed. Finally, we convert the volume from liters to milliliters.
To make a 0.25M solution of ammonium sulfate at a concentration of 6M, you would need to dilute the 6M solution. Assuming you have 1 liter of the 6M solution, you can calculate the volume needed for dilution using the formula: (C1V1 = C2V2), where C1 = 6M, V1 = volume of the 6M solution (in liters), C2 = 0.25M, and V2 = total volume of the diluted solution (in liters). Once you have the volume, you can convert it to grams using the molar mass of ammonium sulfate.
To calculate the amount of potassium chlorate needed to produce 112.5g of oxygen, you first need to determine the molar ratio between potassium chlorate and oxygen. Then, use this ratio to convert the grams of oxygen to grams of potassium chlorate using the molar masses of each compound.
The formula for the ionic compound composed of calcium and chlorate is Ca(ClO3)2. Calcium is a group 2 element with a 2+ charge, and the chlorate ion (ClO3-) has a 1- charge. To balance the charges, two chlorate ions are needed for each calcium ion.