In this reaction, what is the correct coefficient for hydrogen gas? ? h2 + ? o2 ? ? h2o

1 answer:

6 0

To balance a chemical reaction, it is important to remember that the number of atoms of each element in the reactants and the product side should be equal. This is to follows the law of conservation of mass where mass cannot be created or destroyed. So, the total mass that is used to react should have the same value of the total mass of the substances produced from the reactants. The balanced chemical reaction would be written as follows:

<span> 2h2 + o2 = 2h2o

Reactant = Product
H = 4 = 4
O = 2 = 2

Therefore, the correct coefficient for the hydrogen gas would be 2.</span>

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What volume of a 6.67 m nacl solution contains 3.12 mol nacl??

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You just need to follow this formula:

C = n / V

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If 0.250 mol of hydrogen gas occupies 0.333L at 20.0c what is the pressure in atmospheres?

maria [59]

Answer: The pressure will be 18.05 atm.

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$PV=nRT$

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n = Number of moles of gas = 0.250 moles

R = Universal gas constant = $0.082057\text{ L atm }mol^{-1}K^{-1}$

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4 years ago

Lakshmi has a sample of ammonium nitrate (NH4NO3) that has a mass of 40. 10 g. She knows that the molar mass of NH4NO3 is 80. 04

nexus9112 [7]

Moles are an estimation of the smallest unit of the molecules and the atoms in a sample. The moles of ammonium nitrate in a sample are 0.5010 moles.

<h3>What are moles?</h3>

Moles are calculated by dividing the mass of the substance in gm by that of the molar mass in gram per mole.

Given.

Mass of ammonium nitrate = 40.10 gm

The molar mass of ammonium nitrate = 80. 0432 g/mol

Moles of ammonium nitrate are calculated as:

$\begin{aligned}\rm moles &= \rm \dfrac{mass}{molar\; mass}\\\\&= \dfrac{40.10}{80.0432}\\\\&= 0.5010 \;\rm mol\end{aligned}$