Write the formula of the compound.
Write the numbers of each atom in the formula. Insert the relative atomic mass for each type of atom. Calculate the total mass for each element.
Add up the total mass for the compound.
Answer:
Explanation:
You can deal with this question using two different but related approachs.
1) <u>First approach: 1 mole of gas at 1 atm and 0°C occupy 22.4 liter</u>.
With that you can set a proportion:
- 1 mole / 22.4 liter = 2.00 / V
⇒ V = 2.00 mole × 22.4 liter / 1 mole = 44.8 liter.
<u>2) Second approach: use ideal gas equation:</u>
⇒ V = nRT / p
- V = 2.00 moles × 0.0821 atm-liter / K-mol × 273.15 K / 1 atm = 44.85 liter ≈ 44.9 liter.
There, the two calculations yield the same result, although the second one is more accurate only if you need to use 3 or more significant digits, which is not correct in this case.
If you measure the presure as 1.0 atm (two significant digits) and the temperature as 0.0 °C (two significant digits), the volume must be resported with two significant digits, which yileds to the same result with both calculations: 45 liter.
Answer:
C
Explanation:
like charges repel each others so if they have the same charge they will move away from each other
Answer:
rate = k [H2O] [NO]²
Explanation:
[H2] (M) [NO] (M) Rate (M/s)
Trial 1 0.35 0.30 2.835 x 10-3
Trial 2 0.35 0.60 1.134 x 10-2
Trial 3 0.70 0.60 2.268 x 10-2
Comparing Trial 1 and 2 , the rate of the reaction increases by a factor of 4 when the concentration of NO was doubled. This means that the reaction is second order with respect to NO
Comparing Trial 2 and Trial 3, the rate of reaction increased by a factor of 2 when the concentration of H2O was doubled. This means that the reaction is first order with respect to H2O
The rate law fr the reaction is given as;
rate = k [H2O] [NO]²