Methane reacts with steam to form #"H"_2# and #"CO"# as shown. What volume of #"H"_2# can be obtained from #"100 cm"^3# of methane at STP?
#"CH"_4 + "H"_2"O" -> "CO" + 3"H"_2#
What volume of #"H"_2# can be obtained from #"100 cm"^3# of methane at STP?
a)100 cm³ b) 150cm³ c) 300cm³ d)200cm³
What volume of
a)100 cm³ b) 150cm³ c) 300cm³ d)200cm³
The trick here is to realize that when two gases that take part in a chemical reaction are kept under the same conditions for pressure and temperature, their mole ratio in the balanced chemical equation is equivalent to a volume ratio.
The balanced chemical equation that describes your reaction looks like this
This means that your sample of methane will produce
The molar volume of a gas at STP tells you the volume occupied by one mole of an ideal gas kept under STP conditions. In your case, the volume of methane gas
will contain
under STP conditions. This means that your reaction will produce
If the sample of hydrogen gas is kept under STP conditions, its volume will be equal to
Convert this back to cubic centimeters to get
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The balanced chemical equation for the reaction is:
CH4(g) + 2H2O(g) -> CO2(g) + 4H2(g)
According to the stoichiometry of the reaction, 1 mole of methane produces 4 moles of hydrogen gas.
The molar volume of any ideal gas at STP is 22.4 L (or 22,400 cm^3) per mole.
So, to find the volume of hydrogen produced from 100 cm^3 of methane, we need to calculate the number of moles of methane, then use the stoichiometry to find the number of moles of hydrogen, and finally convert the moles of hydrogen to volume.
1 mole of methane occupies 100 cm^3. Therefore, 1 mole of methane occupies (100/22,400) = 0.004464 moles.
According to the stoichiometry of the reaction, 1 mole of methane produces 4 moles of hydrogen gas. So, 0.004464 moles of methane will produce (4 * 0.004464) = 0.017856 moles of hydrogen gas.
Now, to find the volume of hydrogen gas produced: 0.017856 moles of hydrogen gas will occupy (0.017856 * 22,400) = 399.9744 cm^3.
Therefore, approximately 400 cm^3 of hydrogen gas can be obtained from 100 cm^3 of methane at STP.
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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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