Density is calculated as mass divided by volume.
Step one:
Convert m³ to ml.
1 m³ = 1,000,000 ml
0.250 m³ x 1,000,000 = 250,000 ml
Step two: Convert mg to g.
1 mg = 0.001 g, hence 4.25 x 10^8 mg equals 0.459 g.
Consequently, the density comes out to be 0.459 g/250,000 = 1.836 x 10^-6 g/ml.
Answer:
The temperature of a vessel at a pressure reading of 1.250 atm is 296.43 K.
Explanation:
At standard temperature and pressure (STP), the temperature is valued at 273.15 K with a pressure of 1.000 atm.
If the pressure is measured as 1.250 atm at temperature T.
Applying Gay Lussac's law:
(When volume is constant)
At a pressure of 1.250 atm, the temperature of the vessel is 296.43 K.
Hello! We have the following information: m1 (mass of solute) = 20 % m/m; M1 (molar mass of solute) (NH4)2SO4 =?; m2 (mass of solvent) =? (in Kg). To begin, we determine the solute mass (m1), knowing that: 20% m/m = 20g/100mL implies 20 → 100 mL (0.1 L) implies y g → 1 L. By calculating, y = 20/0.1 gives y = 200 g; thus, m1 = 200 g. Next, let's ascertain the Molar Mass of (NH4)2SO4: N = 2*14 = 28, H = (2*4)*1 = 8, S = 1*32 = 32, O = 4*16 = 64, totaling M1 = 132 g/mol. Now, we must find the mass (m2) of the solvent. The volume of the solvent will be: 1000 - 179 gives V = 821 mL (volume of disolvent). Assuming 1 mL = 1g, then the solvent mass is m2 = 821 g → m2 = 0.821 Kg. Now, we can apply the gathered information to the molality formula.
