Thank you so much men nice well
Maybe 47.999 g if I can’t I’m sorry.
Answer:
it becomes acid
Explanation:
due to discovery of newton
Answer:
Explanation:
The<em> heat</em> to <em>vaporize</em> a l<em>iquid</em> is equal to the amount of liquid in moles multiplied by the specific <em>heat of vaporiztion</em> per mole.
First, calculate the number of moles in 35.5g of <em>butane</em>.
- Molar mass of butane: 58.124 g/mol
- Number of moles = mass in grams/molar mass
- Number of moles = 35.5g / 58.124g/mol = 0.6107632mol
Now, calculate the heat to vaporize that amount of <em>liquid butane</em>:
- Heat = number of moles × specific heat of vaporization
- Heat = 0.6107632mol × 21.3kJ/mol = 13.0 kJ
The answer must be reported with 3 significant figures.
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:
