What mass of water can be obtained from 4.0 g of h2 and 16 g of o2? 2 h2 + o2 > 2 h2o9 g18 g54 g36 g

There will be produced 18.02 grams of H2O

Explanation:

Step 1: Data given

Mass of H2 = 4.0 grams

Mass of O2 = 16 grams

Molar mass of O2 = 32 g/mol

Molar mass of H2 = 2.02 g/mol

Molar mass of H2O = 18.02 g/mol

Step 2: The balanced equation

O2 + 2H2 → 2H2O

Step 3: Calculate moles of O2

Moles O2 = mass O2 / molar mass O2

Moles O2 = 16.0 grams / 32. g/mol

Moles O2 = 0.500 moles

Step 4: Calculate moles H2

Moles H2 = 4.0 grams / 2.02 g/mol

Moles H2 = 1.98 moles

Step 5: Calculate limting reactant

For 1 mol of O2 we need 2 moles of H2 to produce 2 moles of H2O

O2 is the limiting reactant. It will completely be consumed. (0.500 moles).

H2 is in excess. There will be react 2*0.500 = 1.00 moles

There will remain 1.98 - 1.00 = 0.98 moles

Step 6: Calculate moles of H2O

For 1 moles of O2 we need 2 moles of H2O

For 0.500 moles of O2 consumed, we'll produce 2*0.500 = 1.00 moles of H2O

Step 7: Calculate mass of H2O

Mass H2O = moles H2O * molar mass H2O

Mass H2O = 1.00 moles * 18.02 g/mol

Mass H2O = 18.02 grams

There will be produced 18.02 grams of H2O

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i