balanced equation =2 H(2)+ 1 O(2) -> 2H(2)O
A. What mass of H2O would be produced from7.4 mg of O2
B. What is the volume of H2O would be produced from 7.4kg of O2. Density of water = 1.000g/ml
2 mol of water --> 2*18 g
1 mol O2 --2*16 g
(2*18/2*16) * 7.4 mg
= 9*7.4/8 = 8.325 mg
7400 grams O2 ---> 8325 grams H2O
---> 8325 mL H2O
or
8.325 liters
To answer these questions, we need to use stoichiometry and some basic calculations. Let's go step by step:
A. What mass of H2O would be produced from 7.4 mg of O2?
1. Start by converting the mass of O2 to the number of moles. To do this, we need to know the molar mass of O2. Oxygen (O) has a molar mass of approximately 32 g/mol. Therefore, O2 has a molar mass of 2 x 32 g/mol = 64 g/mol.
Mass of O2 = 7.4 mg = 7.4 x 10^(-3) g
Number of moles of O2 = Mass / Molar mass = 7.4 x 10^(-3) g / 64 g/mol
2. Use the balanced equation to determine the stoichiometric ratio between O2 and H2O. According to the balanced equation, 1 mole of O2 will produce 2 moles of H2O.
Moles of H2O produced = (Moles of O2) x (Coefficient of H2O / Coefficient of O2)
Moles of H2O produced = (7.4 x 10^(-3) g / 64 g/mol) x (2 / 1)
3. Convert moles of H2O to mass. The molar mass of water (H2O) is approximately 18 g/mol.
Mass of H2O produced = Moles of H2O x Molar mass of H2O
Mass of H2O produced = (7.4 x 10^(-3) g / 64 g/mol) x 18 g/mol
Therefore, the mass of H2O produced from 7.4 mg of O2 is:
Mass of H2O = (7.4 x 10^(-3) g / 64 g/mol) x 18 g/mol
B. What is the volume of H2O produced from 7.4 kg of O2?
1. Convert the mass of O2 from kg to g:
Mass of O2 = 7.4 kg x 1000 g/kg = 7400 g
2. Determine the number of moles of O2 using the molar mass of O2 (64 g/mol) as mentioned in part A.
Number of moles of O2 = Mass / Molar mass = 7400 g / 64 g/mol
3. Use the balanced equation to find the stoichiometric ratio between O2 and H2O, as we did in part A.
Moles of H2O produced = (Moles of O2) x (Coefficient of H2O / Coefficient of O2)
Moles of H2O produced = (7400 g / 64 g/mol) x (2 / 1)
4. Calculate the volume of H2O produced from the moles of H2O. Since we are given the density of water (1.000 g/mL), we can use the formula:
Volume (mL) = Mass (g) / Density (g/mL)
Volume of H2O = (Moles of H2O x Molar mass of H2O) / Density of water
Therefore, the volume of H2O produced from 7.4 kg of O2 is:
Volume of H2O = ((7400 g / 64 g/mol) x 18 g/mol) / 1.000 g/mL
By substituting the values and performing the necessary calculations, you will get the final answers.