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From the stoichiometry of the reaction, we can see that the volume of carbon monoxide reacted is 44.8 L.
<h3>What is stoichiometry?</h3>
Stoichiometry is used to obtain the amount of substance reacted or the amount of product formed.
Number of moles of CO2 in 88g = 88g/4 g/mol = 2 moles
Molar mass of carbon monoxide = 12 + 16 = 28g/mol
We can see that 1 mole of oxygen was used in the reaction hence the mass of oxygen used is 32 g/mol. Given the stoichiometry of the reaction, 28g of carbon monoxide was burned.
If 1 mole of a gas occupies 22.4 L
2 moles of a gas occupies 2 moles * 22.4 L/1 mole
= 44.8 L
Learn more about stoichiometry:brainly.com/question/9743981
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Answer:
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Explanation:
Answer:
Amount of sugar in solution = 82.5 gram
Explanation:
Given:
Sugar in solution percentage = 15%
Total solution = 550 grams
Find:
Amount of sugar in solution
Computation:
Amount of sugar in solution = Sugar in solution percentage x Total solution
Amount of sugar in solution = 15% X 550
Amount of sugar in solution = 82.5 gram
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).
