Question:
At standard temperature and pressure, the volume of a tire is 3.5L. What is the new pressure if the temperature outside is 296k and its weight causes the volume of the gas is 2.0 L?
Answer:
The new pressure is: 1.896 atm
Explanation:
At standard temperature and pressure, we have:
Outside, we have:
Required
Determine the new pressure
Using combined gas law, we have:
This gives:
Solve for 
Xe is bigger:)
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<span>The following acids do NOT ionize completely in solution because they are not strong acids are as follows:
a HBr
b HI
c H2SO3
d H3N
e HNO2
f HF
</span>
Answer:
OptionA. 2C4H10 + 13O2 —> 8CO2 + 10H20
Explanation:
Butane burns is air (O2) according to the equation:
C4H10 + O2 —> CO2 + H20
Considering the equation, it is evident that it not balanced. Now let us balance the equation as shown below;
There are a total of 4 carbon atoms on the left and 1 carbon atom on the right. It can be balanced by putting 4 in front of CO2 as shown below:
C4H10 + O2 —> 4CO2 + H20
Next, there are 10 hydrogen atoms on the left and 2 hydrogen atoms on the right. Therefore to balance it, put 5 in front of H2O as shown below:
C4H10 + O2 —> 4CO2 + 5H20
Now, there are a total of 13 oxygen atoms on the right and 2 at the left. To balance it, put 13/2 in front of O2
as shown below
C4H10 + 13/2O2 —> 4CO2 + 5H20
Now we multiply through by 2 clear off the fraction and we obtained:
2C4H10 + 13O2 —> 8CO2 + 10H20
