32g of oxygen is required to burn 4g of hydrogen.
Define molecular mass.
A specific molecule's mass is expressed in daltons and is known as the molecular mass (m) (Da or u). Due to the varying isotopes of an element that they contain, multiple molecules of the same substance can have distinct molecular weights.
The total atomic mass of every atom in a molecule, calculated using a scale with hydrogen, carbon, nitrogen, and oxygen having atomic masses of 1, 12, 14, and 16, respectively. For instance, water has a molecular mass of 18 (2 + 16), which consists of two hydrogen atoms and one oxygen atom. known also as molecular weight.
In ,2H2+O2-----> 2H2O
H 2 molecules have a mass of 2 g/mol.
The molecular weight of oxygen is 32 g/mol.
When the chemical equation is balanced,
To totally react, 32 g of oxygen are needed for every 22=4 g of hydrogen.
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An increase in kinetic energy corresponds to an increase in temperature. Out of boiling, condensation, freezing, and precipitation, boiling is the only one that indicates an increase in temperature.
Answer:
Explanation:
molar mass of BaCl2 = 208.23
mol of BaCl2 = 8/208.22
mol of BaCl2 = 0.03841905
Molarity = 0.03841905/0.450
Molarity = 0.085 M
Answer:
22.9 Liters CO(g) needed
Explanation:
2CO(g) + O₂(g) => 2CO₂(g)
? Liters 32.65g
= 32.65g/32g/mol
= 1.02 moles O₂
Rxn ratio for CO to O₂ = 2 mole CO(g) to 1 mole O₂(g)
∴moles CO(g) needed = 2 x 1.02 moles CO(g) = 2.04 moles CO(g)
Conditions of standard equation* is STP (0°C & 1atm) => 1 mole any gas occupies 22.4 Liters.
∴Volume of CO(g) = 1.02mole x 22.4Liters/mole = 22.9 Liters CO(g) needed
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*Standard Equation => molecular rxn balanced to smallest whole number ratio coefficients is assumed to be at STP conditions (0°C & 1atm).
