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How is hfusion used to calculate the energy required to vaporize a volume of liquid?
Liters liquid 1000ml/1L g/ml mol/g Hfusion
What mass of KCl is required to prepare 383.00 mL of 0.500 M solution?
I'll go straight to the equation, to prepare 0.5 M of KCl in 383 ml, simply calculate it this way, *Molar mass of KCl is 74.5513 g/mol *0.5 M is also known as 0.5 mol/Litre 74.5513 g/mol x 0.5 mol/litre x 0.383 Litre = 14.2766 g So, you need 14.2766 g of KCl to prepare 0.5 M in 383 ml solution.
Please show work How many moles would there be in 300 ml of of a 1.5 M solution?
300 (mL) * 1.5 (mol/L) * 1 (L) / 1000 (mL) = 0.45 mol
How do you calculate 1.51 mol of aluminum?
35
What mass of KI is present in 276 mL of a 0.50 M solution?
V*c*M = 276(mL)*0.001(L/mL)*0.50(mol KI/L)*166.0(g KI/mol KI) = 22.9 g KI
Calculate the molarity of a solution of potassium permanganate and density is 1.04 gmL which contans 15.00 percent by mass?
C [mol/L] = w% * rho [g/mL] *1000 [mL/L] / (100% * M [g/mol] ) = = w% * rho [g/mL] *10 [mL/L%] / ( M [g/mol] ) = = 15.00 % * 1.04 [g/mL] *10 [mL/L%] / ( 158.034 [g/mol] ) = = 0.987 [mol/L] the molarity of the solution of potassium [in mol per liter] equals the content of KMnO4 by mass in percents multiply by density in g/mL multiply by 10 [mL/(L*%)] divide by molar mass of KMnO4 (M = 158.034 g/mol) This gives 0.987 mol/L. Thus the molarity equals approximately 1 M.
How many milliliter is 80mg?
ml is a size for an amount of fluid. mg is a size for a mass. You can convert ml in mg if you know the material your dealing with. Then you need the periodic system of elements and calculate the molecular weight of you material knowing; mol(n) = mass(mg) / molecular weight(g) then calculate the volume (ml) =mol(n) / concentration(c)
How is hfusion used to calculate the energy required to vaporize a volume of liquid?
Liters liquid 1000ml/1L g/ml mol/g Hfusion
How is the Hfusion used to calculate the energy required to vaporize a volume of liquid?
Liters liquid 1000ml/1L g/ml mol/g Hfusion
Calculate the volume of a 0.05000 mol/l stock solution of CuSO4 (aq) required to prepare 100.0 ml of a 0.005000 mol/l solution?
For starters, you know that 0.05000-mol L − 1 solution of copper(II) sulfate contains 0.05000 moles of copper(II) sulfate, the solute, for every 1 L = 10 3 mL of the solution.
How much energy does it take to boil 100 mL of water (Refer to table of constants for water.)?
100 mL × × × 40.65 kJ/mol = 226 kJ
What mass of KCl is required to prepare 383.00 mL of 0.500 M solution?
I'll go straight to the equation, to prepare 0.5 M of KCl in 383 ml, simply calculate it this way, *Molar mass of KCl is 74.5513 g/mol *0.5 M is also known as 0.5 mol/Litre 74.5513 g/mol x 0.5 mol/litre x 0.383 Litre = 14.2766 g So, you need 14.2766 g of KCl to prepare 0.5 M in 383 ml solution.
How many mL of water should be added to 50.0 mL of a 15.0 M H2SO4 solution to give a final concentration 300m?
2.5 0.05 L (50 mL) * 15 Mol/L= 300 Mol/L * X litres (0.05 L * 15 Mol/L) / 300 Mol/L = 0.0025 L or 2.5 mL
How is the Hfusion used to calculate volume of liquid frozen that produces 1 kJ of energy?
1kJ 1/Hfusion g/mol ml/g liquid
Please show work How many moles would there be in 300 ml of of a 1.5 M solution?
300 (mL) * 1.5 (mol/L) * 1 (L) / 1000 (mL) = 0.45 mol
What is the number of moles of NaOH in 16.5 mL of 0.750 Molar NaOH?
0.0165 (L) * 0.750 (mol/L) = 0.0124 mol NaOH in 16.5 mL
.25 g of zinc reacted with 10 mL of HCl what is the moles of zinc reacted?
*first you set the equation: -(10mL of HCl)(1 mol of HCl)/(22.4 mL of HCl)= .446 mol of HCl *you divide by the volume of HCl which is 22.4 at STP. *Then you will divide that .446 mol of HCl with the mol of Zn, which is 1: -(.446 mol of HCl)( I mol of Zn)/(1 mol of HCl)= .446 mol Zn
