Answer: First, here is the balanced reaction: 2C4H10 + 13O2 ===> 8CO2 + 10H2O.
This says for every mole of butane burned 4 moles of CO2 are produced, in other words a 2:1 ratio.
Next, let's determine how many moles of butane are burned. This is obtained by
5.50 g / 58.1 g/mole = 0.0947 moles butane. As CO2 is produced in a 2:1 ratio, the # moles of CO2 produced is 2 x 0.0947 = 0.1894 moles CO2.
Now we need to figure out the volume. This depends on the temperature and pressure of the CO2 which is not given, so we will assume standard conditions: 273 K and 1 atmosphere.
We now use the ideal gas law PV = nRT, or V =nRT/P, where n is the # of moles of CO2, T the absolute temperature, R the gas constant (0.082 L-atm/mole degree), and P the pressure in atmospheres ( 1 atm).
V = 0.1894 x 0.082 x 273.0 / 1 = 4.24 Liters.
Explanation:
Answer:
1) 7.256 mol Br2 (Cl2)/(Br2)
The Br2 cancels out, so we have 7.256(2)
This is 14.512.
2) Number of moles = mass / molar mass
Number of moles = 239.7 g/ 35.5 g/mol
Number of moles = 6.8 mol
BrCl=13.6 mol
13.6(11.5.357)
1568.9 g
3) Repeat the same process with problem 2, given that there are 6.022x10^23 atoms in a mole.
Explanation:
Br2 + Cl2 → 2BrCl
The units tell you:
g/cm³ = Mass (in grams) per (divided by) Volume (in cm³);
So:
109/24 = 4.54166..... ⇒ 4.54 g/cm³.
Always look at the units.
Just like for speed, you might have m/s so this is:
Distance (in meters) per (divided by) Time (in seconds).
When 400 J of heat are slowly added to 10 mol of an ideal monatomic gas, its temperature rises by 10°C. The work done on the gas is 845J.
The amount of work done on gas depends upon the internal energy change and the heat supplied to the system.
According to First Law of Thermodynamics, the change in internal energy is equal to the work done and the heat supplied to the system.
This is given by:
ΔU = W + Q
where, ΔU is change in Internal energy
W is the Work done
Q is the heat supplied
Given,
Q = 400J
Number of moles, n = 10
Change in temperature, ΔT = 10°C
Cv = 3/2R ; Since, the given gas is monoatomic (R=8.3)
We know that, ΔU = n Cv ΔT
On substituting the values in above formula,
ΔU = 10 × 3/2 × 8.3 × 10
ΔU = 1245J
Using,
ΔU = W + Q
1245J = W + 400
W = 845J
Hence, the work done on the gas is 845J.
Learn more about Thermodynamics here, brainly.com/question/1368306
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Some examples of amorphous solids include rubber, plastic, and gels. Glass is a very important amorphous solid that is made by cooling a mixture of materials in such a way that it does not crystallize. Glass is sometimes referred to as a supercooled liquid rather than a solid.
