Answer:
0.20 moles
Explanation:
The pressure is proportional to the quantity of gas at a given temperature and volume. So, the quantity needs to be increased by a factor of ...
(35 psi)/(29.2 psi) = 175/146 ≈ 1.19863
The fractional increase required is ...
1.19863 -1 = 0.19863
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The quantity of air currently in the tire is ...
1 mol·519.67°R/(atm·23.6442 L) × (29.2/14.7 atm) × (11.6 L) / (45+459.67)°R
= 1.0035 mol
so we need to add ...
(fraction to add) × (current quantity) = amount to add
0.19863 × 1.0035 mol = 0.1993 mol = amount to add
About 0.20 moles of air must be added to the tire to bring the pressure up.
Mass number is the mass number of that particular Element found in the periodic table and the atomic number is the atomic no. Again found in the periodic table
Answer: let me see I gotta do the work first then I’ll give you the answers
Explanation:
Answer:
C. L mol-1 s-1.
Explanation:
Hello,
In this case, a rate law has the following general form:
Whereas r accounts for the rate measured in M/s units, k is the rate constant whose units depends on the order of the reaction, C the concentration of the species in M units, contributing to the rate and x the order of the reaction.
In such a way, since in this case x equals two (second-order rate), the units of k turns out:
Which matches with C. L mol-1 s-1.
Best regards.
The balanced chemical equation will b
N2H4 + 2 H2O2-> N2 + 4H2O
so first of all we have to find the limiting reactant.
so for this
9.24 g H2O2 ( 1 mol / 34.02 g mass of H2O2 )
= 0.27 mol H2O2
Now
6.56 g of N2H4 ( 1mol / 32.06) = 0.20 mol N2H4
so from the above reaction we found 1:2 ratio of the reactants
so the limiting reactant is hydrogen peroxide. by using this we will find the amount of N2 produced.
so that will be
<span>0.27 mol H2O2 ( 1 mol N2 / 2 mol H2O2 ) ( 14.01 g N2 / 1 mol N2)
=1.89 g N2
hope it helps</span>
