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How many moles are in 100g of KMnO4?
1 mol = 118.94 1 mol / 118.94 = 1.70 / x G = 202.10g
How many moles of KMnO4 are present in 75.0 mL of a 0.0950 M solution?
Molarity = moles of solute/Liters of solution ( 75.0 ml = 0.075 Liters ) Algebraically manipulate, moles of solute = Liters of solution * Molarity Moles KMnO4 = (0.075 Liters)(0.0950 M) = 7.13 X 10 -3 moles KMnO4 ------------------------------------
How many mols in 100g of KMnO4?
0.006327754
How many ml of 0.24M of Na2so4 will be oxidised by 180 ml of 0.32 kmno4 in acid medium?
To find the volume of 0.24M Na2SO4 oxidized by 0.32 kmno4, first calculate the number of moles of KMnO4 using the formula M1V1 = M2V2. Then, use the mole ratio between KMnO4 and Na2SO4 (from the balanced equation) to find the moles of Na2SO4 oxidized. Finally, convert the moles of Na2SO4 to volume using its molarity.
What is the molarity of 0.1 normal KMnO4?
The formula mass of KMnO4 is 158.0Amount of KMnO4 = mass of sample / molar mass = 100/158.0 = 0.633 molThere are 0.633 moles in 100g of potassium permanganate.
How many grams of potassium permanganate KMnO4 are in 2.55 moles?
The compound potassium permanganate has chemical formula KMnO4 Molecular mass of KMnO4 = 39.1 + 54.9 + 4(16.0) = 158.0 Mass of KMnO4 = amount of KMnO4 x Molecular mass of KMnO4 = 2.55 x 158.0 = 403g
How many moles are in 100g of KMnO4?
1 mol = 118.94 1 mol / 118.94 = 1.70 / x G = 202.10g
How many moles of KMnO4 are present in 75.0 mL of a 0.0950 M solution?
Molarity = moles of solute/Liters of solution ( 75.0 ml = 0.075 Liters ) Algebraically manipulate, moles of solute = Liters of solution * Molarity Moles KMnO4 = (0.075 Liters)(0.0950 M) = 7.13 X 10 -3 moles KMnO4 ------------------------------------
How many mols in 100g of KMnO4?
0.006327754
What mass of KMnO4 is required to prepare 3.00 liters of a 0.05253 M solution of KMnO4?
To find the mass of KMnO4 needed, you can use the formula: mass = molarity x volume x molar mass. First, calculate the moles of KMnO4 using moles = molarity x volume. Then, multiply the moles by the molar mass of KMnO4 to find the mass needed.
How many grams of potassium permanganate are in 2.20 moles?
To calculate the grams of potassium permanganate in 2.20 moles, you would need to know the molar mass of potassium permanganate. The molar mass of potassium permanganate (KMnO4) is about 158.034 g/mol. So, 2.20 moles of KMnO4 is equal to 2.20 moles x 158.034 g/mol = 347.67 grams of potassium permanganate.
How many ml of 0.24M of Na2so4 will be oxidised by 180 ml of 0.32 kmno4 in acid medium?
To find the volume of 0.24M Na2SO4 oxidized by 0.32 kmno4, first calculate the number of moles of KMnO4 using the formula M1V1 = M2V2. Then, use the mole ratio between KMnO4 and Na2SO4 (from the balanced equation) to find the moles of Na2SO4 oxidized. Finally, convert the moles of Na2SO4 to volume using its molarity.
Can you dissolve .35 moles of Potassium Permanganate (KMnO4) into 500 mL of water?
The solubility of potassium permanganate in water at 2o 0C is 64 g/l (or 32 g/0,5 L).The molar mass of KMnO4 is 158,034 g and 0,35 moles KMnO4 is equal to 55,312 g.So it is not possible to dissolve o,35 moles KMnO4 in 0,5 L.
A certain amount of hydrogen peroxide was dissolved in 100 ml of water and then titrated with 1.68m kmno4 how much h2o2 was dissolved if the titration required 22.3 ml of the kmno4 solution?
To calculate the amount of hydrogen peroxide (H2O2) dissolved, you can use the equation: moles of KMnO4 = moles of H2O2. Firstly, calculate the moles of KMnO4 (given concentration and volume). Then, use the balanced chemical equation to determine the moles of H2O2, as they have a 1:1 stoichiometric ratio. Finally, convert moles of H2O2 to grams using the molar mass to find the amount dissolved in the solution.
What is the molarity of 0.1 normal KMnO4?
The formula mass of KMnO4 is 158.0Amount of KMnO4 = mass of sample / molar mass = 100/158.0 = 0.633 molThere are 0.633 moles in 100g of potassium permanganate.
If you have 17.34 moles of potassium permanganate how many kilograms of the substance do you have?
Potassium permanganate = KMnO4 Molar mass of KMnO4 K = 1 * 39.10 g = 39.10 g Mn = 1 * 54.94 g = 54.94 g O = 4 * 16.00 g = 64.00 g Total = 158.04 g/mol 17.34 mol KMnO4 * (158.04 g/1 mol KMnO4) = 2740.41 g KMnO4 Convert the grams to kilograms. 1 kg = 1000 g 2740.41 g * (1 kg/1000 g) = 2.74041 kg Therefore, 17.34 moles of potassium permanganate is equal to about 2.74 kilograms.
What volume of 0.380 M NaI would be required to oxidize 45.0 ml of 0.500 M KMnO4 in acidic solution?
To determine the volume of 0.380 M NaI needed to oxidize 45.0 mL of 0.500 M KMnO4 in acidic solution, we first calculate the moles of KMnO4: [ \text{Moles of KMnO4} = 0.500 , \text{M} \times 0.045 , \text{L} = 0.0225 , \text{moles} ] In acidic conditions, the balanced reaction shows that 1 mole of KMnO4 reacts with 5 moles of I⁻ (from NaI). Therefore, the moles of NaI required are: [ \text{Moles of NaI} = 5 \times 0.0225 = 0.1125 , \text{moles} ] Now, using the concentration of NaI, we can find the volume needed: [ \text{Volume of NaI} = \frac{0.1125 , \text{moles}}{0.380 , \text{M}} \approx 0.296 , \text{L} \text{ or } 296 , \text{mL} ] Thus, approximately 296 mL of 0.380 M NaI is required.
