#"1423 g C"_2"H"_7"N"# undergoes incomplete combustion. What mass of #"CO"# and #"H"_2"O"# can be produced? The equation is:
#"4C"_2"H"_7"N"+13"O"_2→8"CO"+14"H"_2"O"+4"NO"#
The mass of
The mass of
Equation in balance
This kind of question follows a pattern:
- Mol product to mol reactant
- Mol product to mol reactant
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To determine the mass of CO and H2O produced, we need to know the extent of incomplete combustion, typically represented by a mole ratio or percentage yield. Without that information, it's impossible to calculate the exact mass of CO and H2O produced.
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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.
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