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What volume of 2.40 M SrCl2 is needed to prepare 525 ml of 5.00 mM SrCl2?
First, calculate the moles of SrCl2 needed for the 525 ml solution: (0.525 L) x (5.00 mM) = 0.00263 moles. Then, use the molarity formula to find the volume of the 2.40 M SrCl2 solution needed: (0.00263 moles) / (2.40 mol/L) = 0.001096 L = 1.10 ml.
How many formula units are in 0.59 mol of CuSO4?
0.59 * 6.02 * 10^23 = 3.6 * 10^23
How many formula units make up 40.0 g of magnesium chloride (MgCl2)?
To find the number of formula units in 40.0 g of magnesium chloride (MgCl2), first calculate its molar mass. The molar mass of MgCl2 is approximately 95.21 g/mol (24.31 g/mol for Mg and 35.45 g/mol for Cl, multiplied by 2). Next, divide the mass of the sample by the molar mass: 40.0 g ÷ 95.21 g/mol ≈ 0.420 mol. Finally, multiply the number of moles by Avogadro's number (6.022 x 10²³ formula units/mol) to get approximately 2.53 x 10²³ formula units of MgCl2.
How many formula units make up 10.6 g of magnesium chloride?
To find the number of formula units in 10.6 g of magnesium chloride (MgCl₂), first calculate its molar mass. The molar mass of MgCl₂ is approximately 95.21 g/mol. Then, convert grams to moles: (10.6 , \text{g} \div 95.21 , \text{g/mol} \approx 0.111 , \text{mol}). Finally, multiply the moles by Avogadro's number ((6.022 \times 10^{23}) units/mol) to get the number of formula units: (0.111 , \text{mol} \times 6.022 \times 10^{23} \approx 6.69 \times 10^{22}) formula units of magnesium chloride.
How many formula units make up 23.6 g of magnesium chloride?
To determine how many formula units make up 23.6 g of magnesium chloride (MgCl₂), first calculate its molar mass, which is approximately 95.3 g/mol. Next, divide the mass of magnesium chloride by its molar mass: 23.6 g ÷ 95.3 g/mol ≈ 0.247 mol. Since one formula unit of MgCl₂ contains one magnesium atom and two chloride atoms, the number of formula units is Avogadro's number (6.022 x 10²³) multiplied by the number of moles: 0.247 mol x 6.022 x 10²³ ≈ 1.49 x 10²³ formula units.
How many formula units are in 5.33 mol of CuCl2?
A mole of substance contains Avogadros number (6.022 X 1023) formula units or molecules). 5.33 mol will contain 5.33 X 6.022 X1023 = 3.209 X1024
How many formula units make up g of magnesium chloride?
molar mass of MgCl2=95.211g/mol mol=mass/molar mass=34.8g*mol/95.211g=0.3655039859molMgCl2 #of anything=mol*Avogadro's#=0.3655mol*6.022*1023formula units/mol answer= 2.20*1023
How many formula units are there in 0.0482 mol of sodium sulfate?
To determine the number of formula units in 0.0482 mol of sodium sulfate, you first need to find the molar mass of sodium sulfate (Na2SO4). The molar mass of Na2SO4 is approximately 142.04 g/mol. Then, divide the given amount of moles by the molar mass to find the number of formula units. In this case, there are approximately 3.39 x 10^22 formula units in 0.0482 mol of sodium sulfate.
How many formula units of iron (II) oxide are needed to produce 3.6 mol Fe2O3?
7.2
What volume of 2.40 M SrCl2 is needed to prepare 525 ml of 5.00 mM SrCl2?
First, calculate the moles of SrCl2 needed for the 525 ml solution: (0.525 L) x (5.00 mM) = 0.00263 moles. Then, use the molarity formula to find the volume of the 2.40 M SrCl2 solution needed: (0.00263 moles) / (2.40 mol/L) = 0.001096 L = 1.10 ml.
How many formula units make up 21.2 of MgCl2?
To find out how many formula units of MgCl2 are in 21.2g, you can use the formula: (mass in grams)/(molar mass). The molar mass of MgCl2 is 95.211 g/mol. So, (21.2 g)/(95.211 g/mol) = 0.223 moles of MgCl2. Since there is 1 formula unit of MgCl2 in 1 mole, there are 0.223 formula units in 21.2g of MgCl2.
How many formula units are in 0.59 mol of CuSO4?
0.59 * 6.02 * 10^23 = 3.6 * 10^23
How many Cah2 formula units are present in 7.596 g of CaH2?
To find the number of CaH2 formula units in 7.596 g of CaH2, we first calculate the molar mass of CaH2, which is 42.08 g/mol. Then, we use this molar mass to convert the mass to moles (7.596 g / 42.08 g/mol = 0.1804 mol). Finally, we use Avogadro's number to convert moles to formula units (0.1804 mol * 6.022 x 10^23 formula units/mol = 1.09 x 10^23 formula units).
How many formula units make up 40.0 g of magnesium chloride (MgCl2)?
To find the number of formula units in 40.0 g of magnesium chloride (MgCl2), first calculate its molar mass. The molar mass of MgCl2 is approximately 95.21 g/mol (24.31 g/mol for Mg and 35.45 g/mol for Cl, multiplied by 2). Next, divide the mass of the sample by the molar mass: 40.0 g ÷ 95.21 g/mol ≈ 0.420 mol. Finally, multiply the number of moles by Avogadro's number (6.022 x 10²³ formula units/mol) to get approximately 2.53 x 10²³ formula units of MgCl2.
How many formula units are in 5.6 g of H2S?
To calculate the number of formula units in 5.6 g of H2S, you first need to determine the molar mass of H2S, which is 34.08 g/mol. Then, you can use the formula: Number of formula units = (mass given / molar mass) * Avogadro's number. Plugging in the values, you get: (5.6 g / 34.08 g/mol) * 6.022 x 10^23 = 9.89 x 10^22 formula units in 5.6 g of H2S.
How many NaCl formula units does it contain?
0,16 mg NaCl is equivalent to 2,7.10-5 mol.
How many formula units make up 11.6g of mgcl2?
To find the number of formula units of MgCl2 in 11.6g, first calculate the molar mass of MgCl2 (95.21 g/mol). Then, divide the given mass by the molar mass to find the number of moles (0.122 mol). Since 1 mol of MgCl2 contains 1 formula unit, the number of formula units in 11.6g of MgCl2 is also 0.122 mol.
