Suppose that 4.9 mol no2 and 0.40 mol h2o combine and react completely. which reactant is in excess?

1 answer:

4 0

Answer is: NO₂ (nitrogen (IV) oxide) is in excess.

Balanced chemical reaction: 3NO₂(g) + H₂O(l) → 2HNO₃(l) + NO(g).
n(NO₂) = 4.9 mol.
n(H₂O) = 0.4 mol.
From chemical reaction: n(NO₂) :(H₂O) = 1 : 3.
For 0.4 mole of water, we need: 0.4 mol : n(NO₂) = 1 : 3; n(NO₂) = 1.2 mol.
Because we have more than 1.2 moles of nitrogen(IV) oxide, this molecule is in excess.

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How many grams of sulfur trioxide are produced 18 mol O2 react with sufficient sulfur? Show all your work S8 +12O 2> 8SO3

SOVA2 [1]

Answer:

$m_{SO_3}=2.31x10^4gSO_3$

Explanation:

Hello!

In this case, since the reaction between sulfur and oxygen is:

$S_8 +\frac{1}{2} O_2 \rightarrow 8SO_3$

Whereas there is a 1/2:8 mole ratio between oxygen and SO3, and we can compute the produced grams of product as shown below:

$m_{SO_3}=18molO_2*\frac{8molSO_3}{1/2molO_2} *\frac{80.06gSO_3}{1molSO_3} \\\\m_{SO_3}=23,057.3gSO_3=2.31x10^4gSO_3$

Best regards!

7 0

3 years ago

A solution of H2SO4 with a molal concentration of 5.25m has a density of 1.266 g/ml. what is the molar concentration of this sol

Gelneren [198K]

So first find the moles of the H₂SO₄: Mass = Moles x RFM
so mass = 5.25 x 98 = 514.5g of H₂SO₄

so to find how many Liters of solution use:

Volume = Density x Grams of solute (per kg +1000)

density = 1.266 x 514.5 +1000 = 1917.357kg/l

now use equation: Conc. = Moles / Volume of solution to find the conc.
Conc. = 5.25 x 1917.357 = 4.39Mol⁻¹
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6 0

3 years ago

Read 2 more answers

Measurements show that unknown compound X has the following composition:

zvonat [6]

Answer: The empirical formula of X is $C_{5}H_4O_2$ .