Suppose 9.5 g of gaseous C2H2 reacts with excess O2 according to the reaction below. What is the mass of CO2 produced? C2H2(g) + O2(g) → CO2(g) + H2O(ℓ)
According to the stoichiometry, one mole of ethyne is needed to produce two moles of carbon dioxide.
By signing up, you agree to our Terms of Service and Privacy Policy
To find the mass of CO2 produced, first, calculate the moles of C2H2 using its molar mass. Then, use the stoichiometry of the reaction to determine the moles of CO2 produced. Finally, multiply the moles of CO2 by its molar mass to find the mass. The molar mass of CO2 is 44.01 g/mol.
- Calculate moles of C2H2: ( \text{moles} = \frac{\text{mass}}{\text{molar mass}} )
- Use stoichiometry to find moles of CO2 produced.
- Convert moles of CO2 to mass: ( \text{mass} = \text{moles} \times \text{molar mass of CO2} ).
By signing up, you agree to our Terms of Service and Privacy Policy
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- If you have the equation of a reaction, and are told that there is 100grams of each of the reactant, what do you do in order to find which reactant will limit the reaction?
- What is the molecular mass of #NH_3#?
- If 1.75 moles of copper (II) chloride react with 2.00 moles of sodium nitrate, which one is the limiting reactant?
- How many moles of oxygen would have be consumed to produce 68.1 g of water in the reaction #C_3H_8 + 5O_2 -> 3CO_2 + 4H_2O#?
- Using the equation, #"4Fe + 3O"_2##rarr##"2Fe"_2"O"_3#, if 96.0 g of oxygen reacts, what mass of iron was oxidized?

- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7