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3 years ago

What is other word for carefully looking at an object or process beginning with the letter O and is 11 letters long

Chemistry

1 answer:

luda_lava [24]3 years ago

5 0

The word is 'Observation'. It fits the given definition, begins with the letter 'O' and is 11 letters long.

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Hydrocarbons, compounds containing only carbon and hydrogen, are important in fuels. The heat of combustion of cyclobutane, C4H8

Gennadij [26K]

Answer:

1. C4H8 + 6O2 -----> 4CO2 + 4H20

2. 3836.77 kcal

Explanation:

1. Balanced equation for the complete combustion of cyclobutane:

C4H8 + 6O2 -----> 4CO2 + 4H20

2. Heat of combustion of cyclobutane = 650.3 kcal/mol

Molecular weight of cyclobutane, C4H8 = 56.1 g/mol

Mole of C4H8 : mass of cyclobutane/Molecular weight of cyclobutane

Mole of C4H8 = 331/56.1 = 5.9 mol

Energy released during combustion = 5.9 mol × 650.3 kcal/mol = 3836.77kcal

Therefore the energythat is released during the complete combustion of 331 grams of cyclobutane is 3836.77kcal

8 0

3 years ago

What is the empirical formula for a compound composed of 0.0683 mol of carbon ( C ), 0.0341 mol of hydrogen ( H ), and 0.1024 mo

liubo4ka [24]

The empirical formula for a compound composed of 0.0683 mol of carbon ( C ), 0.0341 mol of hydrogen ( H ), and 0.1024 mol of nitrogen ( N ) is $C_2HN_3$ .

<h3>What is the empirical formula?</h3>

An empirical formula tells us the relative ratios of different atoms in a compound.

Given data:

Moles of carbon = 0.0683 mol

Moles of hydrogen = 0.0341 mol

Moles of nitrogen = 0.1024 mol

Dividing each mole using the smallest number that is divided by 0.0341 moles.

We get:

Carbon= 2

Hydrogen=1

Nitrogen=3

The empirical formula for a compound is $C_2HN_3$ .

Learn more about empirical formula here:

brainly.com/question/14044066

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4 0

2 years ago

Determine the heat of reaction (ΔHrxn) for the combustion of ethanol (C2H5OH) by using heat of formation data: C2H5OH (l) + 3 O2

egoroff_w [7]

Answer:

$\Delta H_{rxn}=-1234.782kJ$

Explanation:

$\Delta H_{rxn}=\sum [n_{i}\times \Delta H_{f}^{0}(product)_{i}]-\sum [n_{j}\times \Delta H_{f}^{0}(reactant_{j})]$

Where $n_{i}$ and $n_{j}$ are number of moles of product and reactant respectively (equal to their stoichiometric coefficient).

$\Delta H_{f}^{0}$ is standard heat of formation.

So, $\Delta H_{rxn}=[2mol\times \Delta H_{f}^{0}(CO_{2})_{g}]+[3mol\times \Delta H_{f}^{0}(H_{2}O)_{g}]-[1mol\times \Delta H_{f}^{0}(C_{2}H_{5}OH)_{l}]-[3mol\times \Delta H_{f}^{0}(O_{2})_{g}]$