How many moles of butane do we need to produce 10 moles of CO2 by reaction with oxygen? I think the balanced equation is 2 C4H10 + 13 O2 -----> 8 CO2 + 10 H2O
I appears that we get 2/8 mole carbondioxide for each mole of butane
moles butane=10*2/0=20/8 moles=2.5 moles
oops typo
moles butane=10*2/8=20/8 moles=2.5 moles
To determine the number of moles of butane needed to produce 10 moles of CO2, we can use the balanced equation:
2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O
By inspecting the equation, we can see that the stoichiometric ratio between butane (C4H10) and carbon dioxide (CO2) is 2:8. This means that for every 2 moles of butane, we get 8 moles of CO2.
To find out how many moles of butane are required to produce 10 moles of CO2, we can set up a proportion:
2 moles C4H10 / 8 moles CO2 = x moles C4H10 / 10 moles CO2
Now we can solve for x:
(2/8) = (x/10)
Cross-multiplying:
8x = 20
Dividing both sides by 8:
x = 2.5
Therefore, we need 2.5 moles of butane to produce 10 moles of CO2.
To determine the number of moles of butane required to produce 10 moles of CO2, we can use the balanced equation provided.
The balanced equation is:
2 C4H10 + 13 O2 → 8 CO2 + 10 H2O
From the equation, we can see that 2 moles of butane (C4H10) react to produce 8 moles of CO2. Therefore, the mole ratio of butane to CO2 is 2:8, which simplifies to 1:4.
To find the moles of butane required to produce 10 moles of CO2, we can set up a simple proportion:
1 mole of butane / 4 moles of CO2 = x moles of butane / 10 moles of CO2
Solving for x, we can cross-multiply:
4 moles of CO2 * x moles of butane = 1 mole of butane * 10 moles of CO2
x moles of butane = (1 mole of butane * 10 moles of CO2) / 4 moles of CO2
Simplifying the expression, we get:
x moles of butane = 2.5 moles of butane
Therefore, 2.5 moles of butane are needed to produce 10 moles of CO2 by reacting with oxygen.