Answer:
247.2g
Explanation:
Using the general gas law equation as follows:
PV = nRT
Where;
P = pressure (atm)
V = volume (L)
n = number of moles (mol)
R = gas law constant (0.0821 Latm/molK)
T = temperature (K)
According to the information in this question, a fuel tank contains 150. L (V) of H2 gas at 20.0 atm (P) at 25.0˚C (T)
Temperature = 25°C = 25 + 273 = 298K
Using PV = nRT
20 × 150 = n × 0.0821 × 298
3000 = 24.4658n
n = 3000/24.4658
n = 122.62
n = 122.6mol
Using the formula, mole = mass/molar mass, to find the mass of H2 gas.
Molar mass of H2 = 1.008(2)
= 2.016g/mol
122.6 = mass/2.016
mass = 122.6 × 2.016
mass = 247.2g.
Hey there!:
Mass = 21.09 g
Volume = 6.44 mL
Therefore;
Density = mass / Volume
Density = 21.09 / 6.44
Density = 3.274 g/mL
Answer:
166 g
Explanation:
Step 1: Write the reaction for the obtaining of Fe from magnetite
Fe₃O₄ ⇒ 3 Fe + 2 O₂
Step 2: Calculate the moles corresponding to 120 g of Fe
The molar mass of Fe is 55.85 g/mol.
120 g × (1 mol/55.85 g) = 2.15 mol
Step 3: Calculate the moles of Fe₃O₄ required to produce 2.15 moles of Fe
The molar ratio of Fe₃O₄ to Fe is 1:3. The moles of Fe₃O₄ required are 1/3 × 2.15 mol = 0.717 mol
Step 4: Calculate the mass corresponding to 0.717 moles of Fe₃O₄
The molar mass of Fe₃O₄ is 231.53 g/mol.
0.717 mol × 231.53 g/mol = 166 g
The wick and the wax
Sorry if that was useless, I'm not sure how generalized you were being
