Assuming the water vapor behaves as an ideal gas,
PV = nRT
For conversions, 760 mmHg = 101325 Pa and 1,000 L = 1 m³
(187.5 mmHg)(101325 Pa/760 mmHg)(5 L)(1 m³/1,000 L) = n(8.314 m³Pa/molK)(65+273 K)
Calculating for n,
n = 0.0445 mole of water
Considering the molar mass of water is 18 g/mol,
The mass of the vaporized water = 0.0445 * 18 = 0.8 g of water evaporated
Therefore,
The fraction of water that vaporized = 0.8/1.2 * 100 = 66.7%
6.28 mol O2 × 2 mol H2 / 1 mol O2 = 12.56 moles H2
When examining its electronic configuration, the last digit should be five, suggesting configurations like (2,5), (2,8,5), or (2,8,8,5), among others.
Thus, elements that end with the number 5 in their outer shell include N, P, As, Sb, Bi, Uup. Based on the choices presented, the probable answer is option 4) Phosphorus.
Given that the value of X is 10, the formula for the unknown hydrate of sodium sulfate becomes NaSO4.10 H2O.
Calculation:
Step 1: Determine the moles of Na2SO4 and H2O.
Moles are calculated by dividing mass by molar mass.
Moles of Na2SO4 are calculated as 1.42 divided by 142, resulting in 0.01 moles.
For H2O: The mass of H2O is 3.22 - 1.42 = 1.8 g.
The moles of H2O are then calculated as 1.8 divided by 18, which gives us 0.1 moles.
Step 2: Find the mole ratio by dividing each mole quantity by the smallest amount (0.01).
This leads to Na2SO4 = 0.01/0.01 = 1.
H2O = 0.1/0.01 = 10.
Be mindful of the integer next to each chemical in the equation, as these will be necessary for the stoichiometric calculations that follow:
Molar mass of <span>k[ag(cn)2]: 199 g/mol
Molar mass of Zn(Cn)2: 117.44 g/mol
Avogadro's number: 6.022</span>×10²³ molecules/mol
a.)
35.27 g*(1 mol/199 g)*(1 mol Zn(Cn)₂/ 2 mol K[Ag(CN)₂])*(6.022×10²³ molecules/mol) = 5.34×10²² molecules of Zn(Cn)₂
b.)
35.27 g*(1 mol/199 g)*(1 mol Zn(Cn)₂/ 2 mol K[Ag(CN)₂])*(117.44 g/mol) = 10.41 g of Zn(Cn)₂
