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2.2 mol water = 2.2 (mol) * 18 (g/mol) water = 39.6 (mol*g/mol) = 40 g
18 g/mol = mol mass of H2O = 2*H + 1*O = (2*1 + 16) g/mol
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How much joules are gained by water during evaporation?
It takes 333.51 or 334 joules to evaporate 1 gram of H2O.
How many grams are in 6.3 moles of BH3?
6.3(mol) * 13.83 (g·mol−1)= 87.1 gram BH3
How many moles are there in 237 g of niobium?
Niobium has a atomic weight Ar = 92.9 g mol-1237 g / 92.9 g mol-1 = 2.55 mol
What is the gfm of anhydrous salt?
Based on the category, this answer will refer to sodium chloride, NaCl. Gfm is gram formula mass and is the same thing as molar mass. To find the gram formula mass of NaCl, you add the gram atomic masses (gam) from the periodic table (atomic weights) of the sodium and chlorine atoms in one formula unit. gam Na = 22.99g/mol gam Cl = 35.45g/mol Ggm of NaCl = 22.99g/mol + 35.45g/mol = 58.44g/mol
How many atoms are in 14.500g Cr?
Use this fomula: (m/M)*NA in which m is mass in gram (g), M is molar mass (g/mol) and NA is the Avogadro number (mol^-1)
How much would the freezing point of water decrease if 4 mol of sugar were added to 1g of water?
Adding 4 mol sugar to 1 g (gram) water is impossible !
How much joules are gained by water during evaporation?
It takes 333.51 or 334 joules to evaporate 1 gram of H2O.
How many liters of hydrogen are produced when 117 grams of potassium react with water?
117(g K) * [1.008(g/mol H) / 39.098(g/mol K)] = 3.02 gram hydrogen
In which compound is the percent composition by mass of chlorine equal to 42 percent?
HClO3 (gram-formula mass = 84 g/mol)
How many grams of CO2 will be produced by burning 34.3 gram of C3H8?
[ 34.3(gC3H8) / 44(g/mol C3H8)] * [ 3mol CO2 / 1molC3H8 ] * 44(g/mol CO2) = 103 gram CO2
How do you prepare 0.01 M from 65 percent HNO3?
The molar mass of HNO3 is 63 gram/mol and of water is 18 gram/mol. Lets assume that the density of the HNO3 + water mixture is equal to the density of water at room temperature is 1000 gram/L. 0.01 M is equal to 0.01 mol HNO3 per liter HNO3 + water. Multiplying the molar mass of HNO3 by the molarity shows this is equal to 0.63 gram HNO3 per liter HNO3 + water. Using the density of water shows that this is equal to 0.000063 gram HNO3 per gram water. This is therefore 0.0065 percent by weight. (The assumption that the density of the mixture is approximately equal to that of pure water seems justified because the amount of HNO3 in the mixture is very low) Assuming we start with an initial 65 percent by weight of HNO3 (10.3 M using the same type of calculation), water will need to be added to dilute to 0.0065 percent (0.01M). To find the required amount of water that is added a total and component mass balance can be used. The total mass balance is given by: Mt = M0 + Ma Here, M0 is the initial amount of water + HNO3, Ma is the added amount of (pure) water and Mt is the total mass of the water + HNO3 after adding more water. The component mass balance over HNO3 is given by: xtMt = x0M0 + xaMa= x0M0 Where xt is the final weight fraction of HNO3 in water, x0 is the initial weight fraction in water and xa is the weight fraction of HNO3 in pure water (which is logically equal to zero). Lets say we have a starting mass M0 = 100 gram HNO3 + water with the initial weight fraction x0 = 0.65 gram HNO3 per gram and we want a final weight fraction xt = 0.000065, rearranging for the total weight after having added water to reach this dilution gives: Mt = x0M0/xt = 0.65x100/0.000065 = 1000000 gram HNO3 + water The amount of water which needs to be added then simply follows from: Ma = Mt - M0 = 1000000 - 100 = 999900 gram water
How many moles are in 3.581023?
3,5810e23 is equal to 0,59 mol.
How many mol of water will be produced from combining 4.85 mol of oxygen with excess hydrogen?
Exactly the same number of mols. 1 mol of oxigen atoms produces 1 mol of water molecules.
How many grams are in 6.3 moles of BH3?
6.3(mol) * 13.83 (g·mol−1)= 87.1 gram BH3
Which term is used to represent the mass of 1 mole of molecules of a substance?
This is equal to the molar mass of this substance.
What is the heat of vaporation of water?
Vaporization heat of water: 40.65 kJ/mol or 2257 kJ/kg or 539.423 calories per gram (very outdated units!)
How many gram are in 238 moles of arsenic?
Atomic mass of Arsenic = 74.9g/mol Using the formula: mass = Atomic mass x number of moles mass = 74.9g/mol x 238 mol = 17826.2 grams
