Answer:0.026ml
Explanation:
Details are found in the image attached. We must subtract the saturated vapour pressure of hydrogen gas at the given temperature from the total pressure of the hydrogen gas collected over water to obtain the actual pressure of hydrogen gas and substitute the value obtained into the general gas equation. The dry hydrogen gas has no saturated vapour pressure hence the value is substituted as given. All temperatures must be converted to Kelvin before substitution.
In order for you to calculate
for the mass of ammonium carbonate, you need to know the molar mass of it and
the nitrogen atoms in the compound. Ammonium carbonate has a molar mass of
96.08 grams per mole. There are two nitrogen atoms in ammonium carbonate which
is equal to 28.02 grams per mole. Divide the molar mass of nitrogen to the
ammonium carbonate, 28.02/96.08 x 100, we get 29.16wt% nitrogen.
The answer is: 0.158 mol
You find this by doing:
number of moles (n) = mass (m) / molar mass (M)
n=158.034/25.0
Rust does not have the properties to catch onto flames. However, if you light it on fire, then it would probably catch in flames but not instantly and will not continue to burn unless you have soaked it in oil or flammable object or substance. :) Hope this helps!
Answer:
2 mol NO2
Explanation:
3NO2(g)+H2O(l)→2HNO3(l)+NO(g)
from reaction 3 mol 1 mol
given 11 mol 3 mol
for 3 mol NO2 ----- 1 mol H2O
for x mol NO2 ----- 3 mol H2O
3:x = 1:3
x = 3 *3/1 = 9 mol NO2
So, for 3 mol H2O are needed only 9 mol NO2.
But we have 11 mol NO2. So, NO2 is in excess, and
11 mol NO2 - 9 mol NO2 = 2 mol NO2 will be left after reaction.
